1) A 0.075 g sample of calcium is reacted with excess hydrochloric acid and it produced 48.50 ml of gas that was collected over water. If the atmospheric pressure was 756 mmHg and the temperature was 22.0°C. How many moles of the gas were produced? What value would you calculate for the gas constant, R? Ca (s)+ 2 HC1 (aq) → CaCl2(aq)+ H2 (g)

A sample of gas contains 0.2000 mol of CO(g) and 0.2000 mol of NO(g) and occupies a volume of 15.5 L. The following reaction takes place: 2CO(g) + 2NO(g) → 2CO2(g) + N₂ (9) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = L

A 0.477 mol sample of O gas has a volume of 12.8 L at a certain temperature and pressure. If all this O were converted to ozone (O) at the same temperature and pressure, what is the ozone volume (in liters)?3 O(g) → 2 O(g)

Calculate the volume of oxygen gas produced at 1.80 atm and 23.1°C by the complete decomposition of 19.9 g of potassium chlorate. The balanced equation for the reaction is 2KClO3(s)  → 2KCl(s) + 3O2(g)

3. A 1.75 g sample of magnesium and iron is added to dilute hydrochloric acid, producing 1.1 L of hydrogen gas at 28.5 0C and 765 mmHg. What is the percent composition (by mass) of the original sample to the nearest whole number? (Hint: magnesium and iron react with HCl according to the following equations): Mg(s)+2HCl(aq)→MgCl2 (aq)+H2 (g) Fe(s)+2HCl(aq)→FeCl2 (aq)+H2 (g)

A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH,SO3, with 368.5 mL of a solution of sodium nitrite according to the following equation. NaNO2 + HNH2SO3- N2 + NaHSO4 + H2O Calculate what must have been the molar concentration of the sodium nitrite. M

A student completes the experiment The Universal Gas Constant and obtains the following data for one trial. mass of magnesium (g): Initial gas volume (ml): Final gas volume (ml): Temperature (°C): Atmospheric pressure (inHg): 30.39 Calculate the universal gas constant, R, for this trial. Assume that the water levels inside and outside the eudiometer tube are the same; that is, assume Ah = 0.00 cm water. Give your answer to two decimal places in the units of L-torr-mol-1. K-¹. 1 in Hg = 25.4 mmHg 1 cm water = 0.735559 mmHg 1 mol Mg = 24.305 g Mg on i TABLE D-4 TEMP DEGA C T 0 1 2 3 4 amm 14.579 4.612 4.646 | 4.660 4.714 4.924 4.959 4.9955.031 15.068 5.291 5.329 5.367 5.406 15.445 15.683 5.723 | 5.7645.805 5.146 16.100 1 6.143 6.1866.2306-274 1 6.318 10.6 I 0.7 J L 1 LI 1 4.7484.783 4.818 1 4.853 I 4.888 1 5.104 | 5.141 | 5.178 5.216 | 5.253 5.484 5.523 5.563 1 5.60215.647 I 5.888 | 5.930 | 5.972 1 6.014 1.6. 7_1 5.363 | 6.407 6.453 I 6.498 1 6.823 | 6. 871 6.919 1 6.967 1 1 | 6.544 |…

A reaction between liquid reactants takes place at 33.0 °C in a sealed, evacuated vessel with a measured volume of 20.0 L. Measurements show that the reaction produced 23. g of carbon monoxide gas. Calculate the pressure of carbon monoxide gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answ to 2 significant digits. pressure: ||| atm

A student reacts 0.0975 g of magnesium with 5.00 mL of 3.00 M hydrochloric acid in a eudiometer (gas collection tube). Write a balanced equation for the reaction. What is the limiting reactant? What volume of hydrogen gas (in mL) does the student collect over water at 28.50°C and 778.1 mmHg?

Pre-Laboratory Questions 1) A 0.075 g sample of calcium is reacted with excess hydrochloric acid and it produced 48.50 mL of gas that was collected over water. If the atmospheric pressure was 756 mmHg and the temperature was 22.0°C. How many moles of the gas were produced? What value would you calculate for the gas constant, R? Ca (s)+ 2 HCl (aq) → CaCl2(aq)+ H2 (g)