In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Lithium hydroxide, LİOH, is used in spacecraft to re-condition the air by absorbing carbon dioxide exhaled by astronauts as shown in the reaction: 2 LIOH(s) + CO2(g) → Liz CO3(s){+ H½O(1) What volume of carbon dioxide gas at 21.0 °C and 781 mm Hg could be absorbed by 327 g LIOH? Enter your value in the first box and an appropriate unit of measure in the second box.

A 10.0 L sample of CO2 gas at 25.0 degrees celsius is heated at a constant pressure until the volume has doubled. What is the final ideal temperature of CO2 in degrees celsius?

Please don't provide handwritten solution ....

Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds 2.0 × 10¹¹ kg per year. The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 3.1 kg of solid sulfur and 10.0 atm of oxygen gas at 800. °C into an evacuated 70.0 L tank. The engineer believes K = 0.98 for the reaction at this temperature. Calculate the mass of solid sulfur he expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken in his belief about the value of K, and the consumption of sulfur you calculate may not be what he actually observes. p' kg ☐ x10 ×

When collecting a gas over water it is necessary to correct for the vapor pressure of water in order to determine the pressure of the gas you are collecting. We will do this by using a graph of ln P in mmHg versus 1/T where T is the temperature in Kelvin. The equation is y = -5206.4 x + 20.621 (With an R^2 = 0.9999). If you collect a gas at 26.8 ℃, what is the value of “x” that you want to use in the equation. (Keep the answer for the next question). (Keep extra digits, you do not want to round in the middle of this calculation). Select one:   a. 0.003660992 b. 0.037313433 c. 0.003378378 d. 299.95 e. 0.0273150 f. 273.15 g. None of these h. 0.003333889 i. 0.0027315

For many purposes we can treat ammonia (NH, ) as an ideal gas at temperatures above its boiling point of -33. °C. Suppose the temperature of a sample of ammonia gas is lowered from 13.0 °C to –16.0 °C, and at the same time the pressure is increased by 10.0%. increase x10 Does the volume of the sample increase, decrease, or stay the same? decrease ? stays the same If you said the volume increases or decreases, calculate the percentage change in % the volume. Round your answer to the nearest percent.

PV=nRT R=0.0821 atm•L/mol•K °C + 273.15 = K 1 atm = 760 mmHg Many metals produce hydrogen gas when dropped in water. For example: Ca (s) +2 H20 (1) → Ca(OH)2 (aq) + H2(g) How much hydrogen gas (in liters) would be produced from dropping 5.0 grams of Calcium into an excess of water, at 25°C and 755 mmHg?

Below is the equation for the combustion of methane (CH ). How many liters of HO are formed by the complete combustion of 1.8 grams of methane at 25 °C and 1.0 atm pressure? CH +20, + CO+2 H,0 → '4(g) - 2/g) (g)

Oxygen gas can be prepared by heating potassium chlorate according to the following equation: 2KCIO3(s)2KCI(s) + 302(g) The product gas, O2, is collected over water at a temperature of 25 °C and a pressure of 758 mm Hg. If the wet O2 gas formed occupies a volume of 8.11 L, the number of grams of O, formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.

What is the temperature of 100.0 g of chlorine gas (molar mass = 70.90 g/mol) in a 4.00 L container at 1.0 atm? R= 0.082 L atm/mol K