D) -2 19. 68.1 g solid CaCO3 is mixed with excess HC1. What is the volume of CO₂ will be collected at 0.0 °C, and 1 atm. (Molar mass CaCO3 = 100.08 g/mol, CO₂ = 44.1 g/mol CaCO3 (s) + 2 HCl (aq) → H₂O (1) +CaCl₂ (aq) + CO₂ (g)

Part C A certain gas is present in a 12.0 L cylinder at 4.0 atm pressure. If the pressure is increased to 8.0 atm the volume of the gas decreases to 6.0 L. Find the two constants k;, the initial value of k, and kf, the final value of k, to verify whether the gas obeys Boyle's law by entering the numerical values for k and kç in the space provided. Express your answers to two significant figures separated by a comma. • View Available Hint(s)

1) a) Sulfuric acid, the industrial chemical produced in the greatest quantity each year, is prepared by the reaction of sulfur in the presence of oxygen and water as described in the balanced chemical equation below. Calculate the volume, in ml, of 18.0 M sulfuric acid solution that can be prepared from the reaction of 1850 g of sulfur with 6.50E4ML oxygen gas at 25°C and 0.965atm and plenty of water. 25(solid) + 302 (gas) + 2H20(liquid) > 2H:SO4(aqueous) b. Which substance is the limiting reactant? Explain how you know.

What volume of H2 gas, measured at 9 °C and 722 torr, can be obtained by reacting 8.40 g of zinc metal with 185 mL of 0.425 M HCl?             (6 marks) Zn(s)  +  2 HCl (aq) → ZnCl2(aq)  +  H2(g) (1 atm = 760 torr)

‍‍ C‍6H12O6(aq)+ 2C2H5OH(aq)= 2CO2(g) Fermentation of  750 mL grape juice (density= 1.0g/L)  is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol ‍. Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25 degrees Celcius? (The density of ethanol is 0.79g/L .)

Find the volume in liters of carbon dioxide gas (CO2) produced at 1.00 atm pressure and 25.0 ∘C from 5.37 mL of 1.00 M HNO3(aq) solution with an excess of sodium carbonate (Na2CO3) according to the unbalanced reactionHNO3(aq) + Na2CO3(aq) → NaNO3(aq) + H2O(l) + CO2(g) Give the answer with 3 or more significant figures.

in the following reaction, 27.1 mL of o2(g) is collected over water at 23*C and barometric pressure 751 mmHg. After the reaction, the buret could not be lowered far enough to make the water levels equal in both the burette and beaker. In fact, you measured the difference in water levels to be 34 mm, what must have been the mass of the Ag2O decomposed? (the vapor pressure of water at 23* C is 21.1 mmHg)

How would you answer these questions?

1) a) Sulfuric acid, the industrial chemical produced in the greatest quantity each year, is prepared by the reaction of sulfur in the presence of oxygen and water as described in the balanced chemical equation below. Calculate the volume, in ml, of 18.0 M sulfuric acid solution that can be prepared from the reaction of 1850 g of sulfur with 6.50x10'mL oxygen gas at 25°C and 0.965atm and plenty of water. 25(solid) + 302 (gas) + 2H20(liquid) _-→ 2H2SO4(aqueous) b. Which substance is the limiting reactant? Explain how you know.

Photosynthesis in plants converts carbon dioxide and water into glucose (C6H1206) and oxygen according to the equation below. 6CO2 (g) + 6H20a → C6H1206 (s) + 602 (g) Substance СО2 (8) H20M C6H1206 (s) 02 (g) kJ AH°; (mol -393.5 -285.8 -1273.3 J H° mol. k 213.6 69.9 209.2 205.0 Calculate the AHº, ASº, and AGº. Is the reaction spontaneous at standard conditions?