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Chemical Equations - Chemistry Questions asked by Filo students

Question 1

Calcium ion has a

2 +

charge. Chloride has a 1 - charge. The formula for calcium chloride is

CaCl 2

. Nitrate has a formula and charge of

NO^{3}

- . How would you write \& solve the formula for calcium nitrate?

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Chemical Equations

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Question 2

Horme - Carva Previous

2 \lor

Nex

⊙

Mathematical Skills for the Physical Sciences: Mastery Test 2 Select the correct answer. A certain satelite orbiting Earth nas a speed of abou 17,000 mileshour What is its approximate speed expressed to the cortect number of significant figures in kilameters/second? One kilometer is about

0.62

mile, and there are 3,600 seconds in an hour:

$29 km / s$
$7.6 km / s$
$38, 000, 000 km / s$
$99, 000, 000 km / s$

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Chemical Equations

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Question 3

(i) [Cr(NH₂),Cl₂] = tetraamminedichloridochromium (III) ion; Cr³¹ (3d³) 3d 4p 000XX/XX XXXXXX XX d-sp³ hybrid d'sp hybridisation in [Cr(NH3)4Cl₂ leads to octahedral structure. (ii) [Ni(CN),1² = tetracyanonickelate(II)ion; Ni²+ (3d%) exes: 3d |11|11|11|11|XX| (56/2/1 4s XX dsp² hybrid dsp hybridisation in [Ni(CN), leads to square planar structure. 07. Describe for any two of the following complex ions, the type of hybridisation, shape and magnetic property: (1) [Fe(H₂O)]2+ (ii) [Co (NH3)]³+ () [NICI, (AL. Nos. Fe=26, Co= 27, Ni = 28) As (1) Atomic orbitals of Fe ion 111 sp'd hybridised orbitals of Fe²+ ion Formation of [Fe(H₂O) [CBSE (AD) 2012 Atomic orbitals of Co (III) ion d'sp hybridised orbitals of Co (III) ion Formation of |CẠNH, P* 4p XXXX Atomic orbitals of Ni (II)ion sp hybridised orbitals of Ni (11) 3d Formation of INICI 3d XX= Electron pair from NH, molecule and CI ion 3d 3d Octahedral because of sp'd hybridisation. Paramagnetic, as there are four unpaired electrons present in the complex ion. 3d XX Electron pair from CN ion 3d 4s 3d XX 1!1!1! XX XX 3d 4p sp'd hybrid XXXXXX XXXX Six pairs of electrons from six H₂O molecules 45 d'sp hybrid XX Six pairs of electrons from six NH, molecules 3d op hybridisation leads to octahedral geometry. Diamagnetic, as there is no unpaired electron present in the complex. 4p 4s XX XX XX 4d 4p sp hybridised 4d XX XX XX XX Four pairs of electrons from four CI ions 4d p hybridisation leads to tetrahedral geometry. Paramagnetic, as there are two unpaired electrons. (any two) unds/225 Coordination Compounds

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Question 4

4. Draw a picture of the titration set-up (step 4) including which chemicals are in the flask and which chemicals are in the buret. 5. Sketch the graphs you would expect to see from plotting the results of step

3 c

and

3 d

. Label the axis. 6. Write the balanced redox equation for the titration being carried out in step 6 . Identify the oxidation states of everything in the reaction.

MnO_{4}^{-} + C_{2} O_{4}^{- 2} \to MnO_{2} + CO_{2} MnO_{4}^{-} + C_{2} O_{4}^{- 2} \to Mn^{+ 2} + CO_{2}

[Equation 1] [Equation 2] 7. Write the two half reactions and identify which substance is being reduced and which is being oxidized. 8. A student pipettes

0.5 mL

of an unknown solution of potassium permanganate into a

500 mL

volumetric flask. They then add water up to the line and mix to make a more dilute solution. They then pipette

1 mL

from that solution into a different

500 mL

volumetric flask. They add DI water up to the line and mix. They determine the concentration of that solution is

0.016 μ M

. What is the concentration of the original undiluted solution? Feb 26

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Question 5

33. a) The standard electrode potential

(E^{\circ})

for the cell containing

0.1 M A g

Ag 3,2 + and

4.00 MCu^{2 +}

298 K

are

E^{\circ} Cu^{2 +} / Cu = 0.34 V, E^{0} Ag^{+} / Ag =

+ 0.80 V

. Calculate the cell potential. (Given:

lo g 4 = 0.6021

) b) State the products of electrolysis obtained on the cathode and anode in the following. i. Dilute solution of

H_{2} SO_{4}

with Pt electrodes. ii. Aqueous solution of

AgNO_{3}

with

Ag

electrodes.

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Chemical Equations

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Question 6

Part 4: Other Stoichiometry Problems: Solve each problem using dimensional analysis. Show the cancelling of units. The combustion (burning) of a sample of butane,

C_{4} H_{10}

(lighter fluid) is shown by the chemical reaction below.

2 C_{4} H_{10 (l)} + 13 O_{2 (g)} \dots CO_{2 (g)} + 10 H_{2} O_{(l)}

If the reaction produced 243 grams of water... 14. How many moles of butane were burned? 15. How many grams of butane were burned? 16. How many moles of oxygen gas would be required in this reaction? 17. How many grams of oxygen gas would be required for this reaction? 18. What volume of oxygen gas would be required for this reaction (in liters)? 19. If

89.6

liters of oxygen gas were required in the reaction how many liters of

CO_{2}

would be produced? Don't Forget: 20. There are liters in 1 mole of gas at STP.

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Chemical Equations

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Question 7

Answer the questions below by circling the number of the correct response 1. Given the reaction:

N_{2} + 3 H_{2} \to 2 NH_{2}

, how many moles of 4. Given the reaction:

2 Na + 2 H_{2} O \to 2 NaOH + H_{2}

nitrogen are needed to produce 8 moles of ammonla?

1 What is the total number of moles of hydrogen produced when 4
3 moles of socium react completely?
2
4
1
3
2
4

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Chemical Equations

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Question 8

Given the reaction:

2 CO + O_{2} \to 2 CO_{2}

What is the minimum number of moles of

O_{2}

required to produce one mole of

CO_{2}

? 5. Given the reactioni

N_{2} (g) + 3 H_{2} (g) = 2 NH_{3} (g)

What is the ratio of moles of

H_{2} (g)

consumed to moles of

NH_{2} (g)

$1.0$
$0.25$ groduced?
$2.0$
$0.50$
$3 : 2$
$2 : 3$
$6 : 6$

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Chemical Equations

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Question 9

Given the reaction:

2 NaOH + H_{2} SO_{4} \to Na_{2} SO_{4} + 2 H_{2} O

6. Given the reaction:

(NH_{3})_{2} CO_{3} \to 2 NH_{2} + CO_{2} + H_{2} O

What is the total number of moles of

NaOH

needed to react What is the minimum amount of ammonium carbonate that reacts completely with 2 moles of

H_{2} SO_{4}

? to produce

1.0

mole of ammonia?

1
$0.5$
$0.25$ mole
17 moles
2
4
$0.50$ mole
34 moles

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Chemical Equations

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Question 10

Part A The reaction between carbon tetrachloride,

CCl_{4}

, and water,

H_{2} O

, to form carbon dioxide,

CO_{2}

, and hydrogen chloride,

HCl^{2}

, has a

Δ G^{\circ}

value of

- 232 kJ / mole

, and so is the modynamically favored. But when you mix carbon tetrachloride with water, no change is observed. What is a possib explanation for this? View Available Hint(s) The reaction is not favored themodynamically. It is a slow reaction kinetically. The activation energy of the reaction is too small. The reaction is not spontaneous. Submit Previous Answers Request Answer

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Question 11

Part C

MnO_{2} (s) + 4 H^{+} (a q) + Cu (s) \to Mn^{2 +} (a q) + 2 H_{2} O (l) + Cu^{2 +} (a q)

Express your answer using two significant figures.

Δ G_{r x n}^{\circ} =

kJ

Submit Request Answer

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Chemical Equations

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Question 12

Indicate the half-reaction occurring at Cathode. Express your answer as a chemical equation. Identify all of the phases in your answer.

NO_{3} - (aq) + e^{-} \to NO (g)

A chemical reaction does not occur for this question. Submit Previous Answers Request Answer

x

Incorrect; Try Again; 26 attempts remaining (P) Pearson

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Question 13

Barium sulfide decomposes into its elements when heat and electricity are applied. Which reaction shows the balanced equation for the decomposition?

$Ba_{2} S \to 2 Ba + S$
$2 Ba_{2} S \to 4 Ba + 2 S$
$BaS_{2} \to Ba + S_{2}$
$8 BaS \to 8 Ba + S_{8}$

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Chemical Equations

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Question 14

Which of the following is a strong base:

Stomach Acid, pH 2
Water, $pH 7$
Drain Cleaner, pH 11
Baking Soda, $pH 8$

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Question 15

Balancing Equations PhET The Law of Conservation of Mass states that matter cannot be created or destroyed. This idea became a scientific law because many careful experiments indicated that mass is the same before and after a chemical or physical change. Examine the chemical equation below:

N_{2} + H_{2} \to NH_{3}

1. If you weighed the atoms that appear on the reactant side of the equation, would they have the same mass as the atoms that appear on the product side? Tell how you know. 2. How many atoms of nitrogen appear to be on the reactant side? The product side? 3. How many atoms of hydrogen appear to be on the reactant side? The product side? 4. Do you feel that this equation is currently following the law of conservation of mass? If our written chemical equations do not follow the law of conservation of mass then we will not be able to make predictions about the impact of those reactions in real life. The simulation will help you get started learning how to balance chemical equations so that they follow the Law of Conservation of Mass. 5. Go to www.phet:colorado.edu and find the simulation called Balancing Chemical Equations and play with the simulation until you know what everything does. 6. Reset the simulation. Under tools, select either the balance or the bar graph (if you decide you don't like one, switch to the other at any time). Add one of each substance to the equation. 7. Consider the nitrogen atoms. a. Which side of the reaction needs more nitrogen? (reactant side or product side) b. Without going back to zero, what can you change so that the number of nitrogen atoms on both sides of the equation is the same? 8. Consider the hydrogen atoms. a. Which side of the reaction needs more hydrogen? (reactant side or product side) b. Without going back to zero, what can you change so that the number of hydrogen atoms on both sides of the equation is the same?

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Chemical Equations

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Question 16

N_{2} + H_{2} \to NH_{3}

1. If you weighed the atoms that appear on the reactant side of the equation, would they have the same mass as the atoms that appear on the product side? Tell how you know. The y' dont have the sowne wass 2. How many atoms of nitrogen appear to be on the reactant side? The product side? 3. How many atoms of hydrogen appear to be on the reactant side? The product side? 4. Do you feel that this equation is currently following the law of conservation of mass? If our written chemical equations do not follow the law of conservation of mass then we will not be able to make predictions about the impact of those reactions in real life. The simulation will help you get started learning how to balance chemical equations so that they follow the Law of Conservation of Mass. 5. Go to www.phetcolorado.edu and find the simulation called Balancing Chemical Equations and play with the simulation until you know what everything does. 6. Reset the simulation. Under tools, select either the balance or the bar graph (if you decide you don't like one, switch to the other at any time). Add one of each substance to the equation. 7. Consider the nitrogen atoms. a. Which side of the reaction needs more nitrogen? (reactant side or product side) b. Without going back to zero, what can you change so that the number of nitrogen atoms on both sides of the equation is the same? 8. Consider the hydrogen atoms. a. Which side of the reaction needs more hydrogen? (reactant side or product side) b. Without going back to zero, what can you change so that the number of hydrogen atoms on both sides of the equation is the same?

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Chemical Equations

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Question 17

5. Go to www.phet colorado.edu and find the simulation called Balancing Chemical Equations and play with the simulation until you know what everything does. 6. Reset the simulation. Under tools, select either the balance or the bar graph (if you decide you don't like one, switch to the other at any time). Add one of each substance to the equation. 7. Consider the nitrogen atoms. a. Which side of the reaction needs more nitrogen? (reactant side or product side) b. Without going back to zero, what can you change so that the number of nitrogen atoms on both sides of the equation is the same? 8. Consider the hydrogen atoms. a. Which side of the reaction needs more hydrogen? (reactant side or product side) b. Without going back to zero, what can you change so that the number of hydrogen atoms on both sides of the equation is the same?

Topic:

Chemical Equations

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Question 18

20. Calculate the free energy change of the reaction:

C

(graphite)

+ O_{2} (g) \to CO_{2} (g)

Given,

Δ H = - 30 kJ mol^{- 1}, Δ S = 3 JK^{- 1} mol^{- 1}

300 K

. 21. Write conjugate base for the following acids:

H_{2} CO_{3}

and

HSO_{4} HOC^{-}

Topic:

Chemical Equations

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Question 19

1 CO_{2}

is linear. Explain these on the basis of C (gralate the free energy change of the reaction: Given (graphite)

+ O_{2} (g) \to CO_{2} (g)

21. Write

Δ H = - 30 kJ mol^{- 1}, Δ S = 3 JK^{- 1} mol - 1

300 K

Topic:

Chemical Equations

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Question 20

How many moles of Fe2O3 are produced if 2 moles of O2 react? 4Fe + 3O2 ~ 2Fe2O3

Topic:

Chemical Equations

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1 2 3 4

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