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Chapter 1: Problem 17

\(\mathrm{CaCO}_{3}(s)+2 \mathrm{H}^{+}(a q) \rightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)\) If the reaction above took place at standard temperature and pressure and 150 grams of \(\mathrm{CaCO}_{3}(\mathrm{s})\) were consumed, what was the volume of \(\mathrm{CO}_{2}(g)\) produced at STP? (A) 11 L (B) 22 L (C) 34 L (D) 45 L

Short Answer

Expert verified
The volume of \(\mathrm{CO}_2(g)\) produced at STP is 33.6 L, therefore the option close to this answer is (C) 34 L.

Step by step solution

01

Converting grams to moles

Convert the mass of \(\mathrm{CaCO}_3(s)\) consumed in the reaction from grams to moles using its molar mass. The molar mass of \(\mathrm{CaCO}_3\) is about 100.1 g/mol. So, \(\frac{150 g}{100.1 g/mol} \approx 1.5 moles\).
02

Apply stoichiometry

From the balanced chemical equation, one can observe that one mole of \(\mathrm{CaCO}_3(s)\) produces one mole of \(\mathrm{CO}_2(g)\). So, if 1.5 moles of \(\mathrm{CaCO}_3(s)\) were consumed, then 1.5 moles of \(\mathrm{CO}_2(g)\) must have been produced.
03

Converting moles to litres

The molar volume of any gas at STP (standard temperature and pressure) is 22.4 liters per mole. Therefore, the volume of 1.5 moles of \(\mathrm{CO}_2(g)\) at STP is \(1.5 \times 22.4 L\).

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Most popular questions from this chapter

In which of the following reactions is entropy increasing? (A) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g)\) (B) \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g)\) (C) \(\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightarrow 2 \mathrm{HCl}(g)\) (D) \(2 \mathrm{NO}_{2}(g) \rightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)\)

\(2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)\) Based on the information given in the table below, what is \(\Delta H^{\circ}\) for the above reaction? \(\begin{array}{cc}{\text { Bond }} & {\text { Average bond energy }(\mathrm{kJ} / \mathrm{mol})} \\ {\mathrm{H}-\mathrm{H}} & {500} \\\ {\mathrm{O}=\mathrm{O}} & {500} \\ {\mathrm{O}-\mathrm{H}} & {500}\end{array}\) (A) \(-2,000 \mathrm{kJ}\) (B) \(-500 \mathrm{kJ}\) (C) \(+1,000 \mathrm{kJ}\) (D) \(+2,000 \mathrm{kJ}\)

A gas sample with a mass of 10 grams occupies 5.0 liters and exerts a pressure of 2.0 atm at a temperature of \(26^{\circ} \mathrm{C} .\) Which of the following expressions is equal to the molecular mass of the gas? The gas constant, \(R,\) is \(0.08(\mathrm{L} \times \mathrm{atm}) / \mathrm{mol} \times \mathrm{K}\) ). (A) \((0.08)(299) \mathrm{g} / \mathrm{mol}\) (B) \(\frac{(299)(0.50)}{(2.0)(0.08)} \mathrm{g} / \mathrm{mol}\) (C) \(\frac{299}{0.08} \mathrm{g} / \mathrm{mol}\) (D) \((2.0)(0.08) \mathrm{g} / \mathrm{mol}\)

A 1 -molar solution of a very weak monoprotic acid has a pH of 5. What is the value of \(K_{a}\) for the acid? (A) \(K_{a}=1 \times 10^{-10}\) (B) \(K_{a}=1 \times 10^{-7}\) (C) \(K_{a}=1 \times 10^{-5}\) (D) \(K_{a}=1 \times 10^{-2}\)

$$\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightarrow 2 \mathrm{HI}(g)$$ When the reaction given above takes place in a sealed isothermal container, the rate law is $$\text { Rate }=k\left[\mathrm{H}_{2}\right]\left[\mathrm{I}_{2}\right]$$ If a mole of \(\mathrm{H}_{2}\) gas is added to the reaction chamber and the temperature remains constant, which of the following will be true? (A) The rate of reaction and the rate constant will increase. (B) The rate of reaction and the rate constant will not change. (C) The rate of reaction will increase and the rate constant will decrease. (D) The rate of reaction will increase and the rate constant will not change.
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