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</div><h2>HL Paper 1</h2><div class="question">
<p>Which variable affects the equilibrium constant, <em>K</em><sub>c</sub>?</p>
<p>A. Atmospheric pressure</p>
<p>B. Catalyst</p>
<p>C. Concentration of reactants</p>
<p>D. Temperature</p>
</div>
<br><hr><br><div class="question">
<p class="p1">What is the effect of an increase of temperature on the yield and the equilibrium constant for the following reaction?</p>
<p class="p1">\[\begin{array}{*{20}{l}} {{\text{2}}{{\text{H}}_{\text{2}}}{\text{(g)}} + {\text{CO(g)}} \rightleftharpoons {\text{C}}{{\text{H}}_{\text{3}}}{\text{OH(l)}}}&{\Delta {H^\Theta } = - 128{\text{ kJ}}} \end{array}\]</p>
<p class="p1"><img src="images/Schermafbeelding_2016-09-25_om_12.20.59.png" alt="N10/4/CHEMI/HPM/ENG/TZ0/22"></p>
</div>
<br><hr><br><div class="question">
<p>Which statements explain why a catalyst is used in the Contact process (shown below)?</p>
<p>\[{\text{S}}{{\text{O}}_2}{\text{(g)}} + \frac{1}{2}{{\text{O}}_2}{\text{(g)}} \rightleftharpoons {\text{S}}{{\text{O}}_3}{\text{(g)}}\]</p>
<p>I. A catalyst lowers the activation energy.</p>
<p>II. A catalyst moves the position of equilibrium towards the product.</p>
<p>III. A catalyst allows the same rate to be achieved at a lower temperature.</p>
<p> </p>
<p>A. I and II only</p>
<p>B. I and III only</p>
<p>C. II and III only</p>
<p>D. I, II and III</p>
</div>
<br><hr><br><div class="question">
<p>What is the effect of increasing the temperature in this reaction?</p>
<p style="text-align: center;">CO<sub>2</sub>(g) + H<sub>2</sub>O(l) \( \rightleftharpoons \) H<sup>+</sup>(aq) + HCO<sub>3</sub><sup>−</sup>(aq) Δ<em>H </em>< 0</p>
<p>A. The pH will decrease.</p>
<p>B. The pH will increase.</p>
<p>C. CO<sub>2</sub> pressure will decrease.</p>
<p>D. The equilibrium position will shift to the right.</p>
</div>
<br><hr><br><div class="question">
<p class="p1">Which statement is correct for the equilibrium \({{\text{H}}_2}{\text{O(l)}} \rightleftharpoons {{\text{H}}_2}{\text{O(g)}}\) in a closed system at 100 °C?</p>
<p class="p1">A. <span class="Apple-converted-space"> </span>All the \({{\text{H}}_{\text{2}}}{\text{O(l)}}\) molecules have been converted to \({{\text{H}}_{\text{2}}}{\text{O(g)}}\).</p>
<p class="p1">B. <span class="Apple-converted-space"> </span>The rate of the forward reaction is greater than the rate of the reverse reaction.</p>
<p class="p1">C. <span class="Apple-converted-space"> </span>The rate of the forward reaction is less than the rate of the reverse reaction.</p>
<p class="p1">D. <span class="Apple-converted-space"> </span>The pressure remains constant.</p>
</div>
<br><hr><br><div class="question">
<p class="p1">Consider the following reversible reaction.</p>
<p class="p1">\[{\text{C}}{{\text{r}}_2}{\text{O}}_7^{2 - }{\text{(aq)}} + {{\text{H}}_2}{\text{O(l)}} \rightleftharpoons {\text{2CrO}}_4^{2 - }{\text{(aq)}} + {\text{2}}{{\text{H}}^ + }{\text{(aq)}}\]</p>
<p class="p1">What will happen to the position of equilibrium and the value of \({K_{\text{c}}}\) when more \({{\text{H}}^ + }\) ions are added at constant temperature?</p>
<p class="p1"><img src="images/Schermafbeelding_2016-10-13_om_18.16.09.png" alt="M09/4/CHEMI/HPM/ENG/TZ1/24"></p>
</div>
<br><hr><br><div class="question">
<p>The enthalpy change for the dissolution of NH<sub>4</sub>NO<sub>3</sub> is +26 kJ mol<sup>–1</sup> at 25 °C. Which statement about this reaction is correct?</p>
<p>A. The reaction is exothermic and the solubility decreases at higher temperature.</p>
<p>B. The reaction is exothermic and the solubility increases at higher temperature.</p>
<p>C. The reaction is endothermic and the solubility decreases at higher temperature.</p>
<p>D. The reaction is endothermic and the solubility increases at higher temperature.</p>
</div>
<br><hr><br><div class="question">
<p>What occurs when the pressure on the given equilibrium is increased at constant temperature?</p>
<p style="text-align: center;">N<sub>2</sub>(g) + O<sub>2</sub>(g) \( \rightleftharpoons \) 2NO(g) Δ<em>H </em>= +180 kJ</p>
<p>A. <em>K</em><sub>c</sub> increases and the position of equilibrium moves to the right.</p>
<p>B. <em>K</em><sub>c</sub> stays the same and the position of equilibrium is unchanged.</p>
<p>C. <em>K</em><sub>c</sub> stays the same and the position of equilibrium moves to the left.</p>
<p>D. <em>K</em><sub>c</sub> decreases and the position of equilibrium moves to the left.</p>
</div>
<br><hr><br><div class="question">
<p>Which of the following will shift the position of equilibrium to the right in the Haber process?</p>
<p> \({{\text{N}}_{\text{2}}}{\text{(g)}} + {\text{3}}{{\text{H}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2N}}{{\text{H}}_{\text{3}}}{\text{(g)}}\) \(\Delta {H^\Theta } = {\text{92.6 kJ}}\)</p>
<p>I. Decreasing the concentration of \({\text{N}}{{\text{H}}_{\text{3}}}{\text{(g)}}\)</p>
<p>II. Decreasing the temperature</p>
<p>III. Increasing the pressure</p>
<p>A. I and II only</p>
<p>B. I and III only</p>
<p>C. II and III only</p>
<p>D. I, II and III</p>
</div>
<br><hr><br>