At which temperature, in K, assuming constant pressure, is the volume of a fixed mass of gas at 127 °C doubled?

A.     200 K

B.     254 K

C.     400 K

D.     800 K

\({\text{300 c}}{{\text{m}}^{\text{3}}}\) of water is added to a solution of \({\text{200 c}}{{\text{m}}^{\text{3}}}\) of \({\text{0.5 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\) sodium chloride. What is the concentration of sodium chloride in the new solution?

A.     \({\text{0.05 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\)

B.     \({\text{0.1 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\)

C.     \({\text{0.2 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\)

D.     \({\text{0.3 mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\)

Four identical containers under the same conditions are filled with gases as shown below. Which container and contents will have the highest mass?

What is the pressure, in Pa, inside a 1.0 m³ cylinder containing 10 kg of H₂ (g) at 25 ºC?

R = 8.31 J K^–1 mol^–1; pV = nRT

A. \(\frac{{1 \times {{10}^4} \times 8.31 \times 25}}{{1.0 \times {{10}^3}}}\)

B. \(\frac{{5 \times {{10}^2} \times 8.31 \times 298}}{{1.0}}\)

C. \(\frac{{1 \times 8.31 \times 25}}{{1.0 \times {{10}^3}}}\)

D. \(\frac{{5 \times {{10}^3} \times 8.31 \times 298}}{{1.0}}\)

A compound with M_r = 102 contains 58.8 % carbon, 9.80 % hydrogen and 31 % oxygen by mass.
What is its molecular formula?

A_r: C = 12.0; H = 1.0; O = 16.0

A. C₂H₁₄O₄

B. C₃H₄O₄

C. C₅H₁₀O₂

D. C₆H₁₄O

Which solution neutralizes 50.0 cm³ of 0.120 mol dm^–3 NaOH (aq)?

A. 12.5 cm³ of 0.080 mol dm^–3 H₃PO₄

B. 25.0 cm³ of 0.120 mol dm^–3 CH₃COOH

C. 25.0 cm³ of 0.120 mol dm^–3 H₂SO₄

D. 50.0 cm³ of 0.060 mol dm^–3 HNO₃

What mass, in g, of hydrogen is formed when 3 mol of aluminium react with excess hydrochloric acid according to the following equation?

\[{\text{2Al(s)}} + {\text{6HCl(aq)}} \to {\text{2AlC}}{{\text{l}}_{\text{3}}}{\text{(aq)}} + {\text{3}}{{\text{H}}_{\text{2}}}{\text{(g)}}\]

A.     3.0

B.     4.5

C.     6.0

D.     9.0

Which coefficients would balance this equation?

__ \({\text{Mn}}{{\text{O}}_2} + \) __ \({\text{HCl}} \to \) __ \({\text{MnC}}{{\text{l}}_2} + \) __ \({\text{C}}{{\text{l}}_2} + \) __ \({{\text{H}}_2}{\text{O}}\)

4.0 g of solid sodium hydroxide is added to \({\text{0.10 d}}{{\text{m}}^{\text{3}}}\) of \({\text{1.0 mol d}}{{\text{m}}^{ - 3}}\) aqueous sulfuric acid.
\[{\text{2NaOH(s) + }}{{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}{\text{(aq) }} \to {\text{ N}}{{\text{a}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}{\text{(aq) + 2}}{{\text{H}}_{\text{2}}}{\text{O(l)}}\]
Which statement is correct?

A.     Neither reactant is in excess.

B.     0.10 mol \({\text{N}}{{\text{a}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\) is formed.

C.     Excess \({{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\) remains in solution.

D.     Excess NaOH remains in solution.

What are the coefficients of \({{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}{\text{(aq)}}\) and \({{\text{H}}_{\text{3}}}{\text{P}}{{\text{O}}_{\text{4}}}{\text{(aq)}}\) when the following equation is balanced using the smallest possible whole numbers?

___ \({\text{C}}{{\text{a}}_3}{{\text{(P}}{{\text{O}}_4}{\text{)}}_2}{\text{(s)}} + \) ___ \({{\text{H}}_2}{\text{S}}{{\text{O}}_4}{\text{(aq)}} \to \) ___ \({\text{CaS}}{{\text{O}}_3}{\text{(s)}} + \) ___ \({{\text{H}}_3}{\text{P}}{{\text{O}}_4}{\text{(aq)}}\)

What volume of carbon dioxide, in dm\(^3\) under standard conditions, is formed when 7.00 g of ethene \(({{\text{C}}_2}{{\text{H}}_4}{\text{, }}{M_{\text{r}}} = 28.1)\) undergoes complete combustion?

A.     \(\frac{{22{\text{.}}4 \times 28{\text{.}}1}}{{7{\text{.}}00}}\)

B.     \(\frac{{22{\text{.}}4 \times 7{\text{.}}00}}{{28{\text{.}}1}}\)

C.     \(\frac{{2 \times 22{\text{.}}4 \times 28{\text{.}}1}}{{7{\text{.}}00}}\)

D.     \(\frac{{2 \times 22{\text{.}}4 \times 7{\text{.}}00}}{{28{\text{.}}1}}\)

Under which conditions does \({\text{C}}{{\text{H}}_{\text{4}}}\) have the same number of molecules as \({\text{100 c}}{{\text{m}}^{\text{3}}}\) of \({{\text{O}}_{\text{2}}}\) at 27 °C and \(1.0 \times {10^5}{\text{ Pa}}\)?

7.102 g of Na₂SO₄ (M = 142.04 g mol^–1) is dissolved in water to prepare \({\text{0.5000 d}}{{\text{m}}^{\text{3}}}\) of solution. What is the concentration of \({\text{N}}{{\text{a}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\) in \({\text{mol}}\,{\text{d}}{{\text{m}}^{ - 3}}\)?

A.     \(2.500 \times {10^{ - 2}}\)

B.     \(1.000 \times {10^{ - 1}}\)

C.     \(1.000 \times 10\)

D.     \({\text{1.000}} \times {\text{1}}{{\text{0}}^{\text{2}}}\)

Which expression gives the sum of all the coefficients for the general equation for the complete

combustion of hydrocarbons?

___ \({{\text{C}}_x}{{\text{H}}_y}{\text{(g)}} + \) ___ \({{\text{O}}_{\text{2}}}{\text{(g)}} \to \) ___ \({\text{C}}{{\text{O}}_{\text{2}}}{\text{(g)}} + \) ___ \({{\text{H}}_{\text{2}}}{\text{O(l)}}\)

A.     \(1 + x + \frac{y}{4}\)

B.     \(1 + x + \frac{y}{2}\)

C.     \(1 + 2x + \frac{{3y}}{4}\)

D.     \(1 + 2x + \frac{{3y}}{2}\)

Which graph represents the relationship between volume and pressure for a fixed mass of gas at constant temperature?