Ethane burns in air to form carbon dioxide and water. The equation is 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)   a) In the above equation, how many liters of oxygen (O2) are required to burn 6.0  L  of ethane (C2H6) gas? Assume that both gases are measured at the same temperature and pressure.   b) In the equation above, what volume of ethane (C2H6) in liters is required to form 28  L  of carbon dioxide (CO2)?   c) In the equation, if 14 L of ethane (C2H6) and 14 L of oxygen (O2) combined and burned to completion, which gas will be leftover after the reaction, and what is the volume of that gas remaining?

A gas is formed in the reaction shown below. The gas laws can help determine the volume of gas produced. Zn(s) + 2 HCl(aq) → ZnCl₂ + H₂(g) Assume that 131.0 grams of Zn was used in this reaction. To determine the number of moles of hydrogen gas formed, you need to know the number of moles of Zn reactant was used. How many moles of Zn were used?

The reaction of Ca(s) with N₂(g) has a percent yield of 68.005% under certain conditions. Assuming excess Ca(s) and STP conditions, how many Liters of N₂(g) are required to produce 3.004 mols of Ca3N₂(s) under the same conditions? 3 Ca(s) + N₂(g) →→→ Ca3N₂(s) • Please report your answer to 2 decimal places. If your last digit(s) is/are a 0 and Canvas drops them, that is okay.

* Question Completion Status: A Moving to another question will save this response. Question 26 SHOW WORK Given the following reaction: CaC 2(s) + 2H 20 - C2H 2(g) + Ca(OH) 2(aq) Assume that you place 1.85 g of calcium carbide in excess water and collect the acetylene gas over water. Calculate the maximum amount of gas that should be produced in grams round answer to 3 decimal places omit trailing zeroes The actual volume of acetylene and water vapor collected is 810 ml at 30.5°C with a pressure of 557.524 mmHg. Calculate the actual amount of gas collected(in grams) round answer to 3 decimal places omit trailing zeroes The vapor pressure of water at 30.5°C is 32.35 mmHg. Calculate the percent yield of acetylene. round answer to 2 decimal places omit trailing zeros A Moving to another question will save this response.

Calculate the volume in milliliters of 3.00 mol/L H₂SO4 required to react with 9.27 g of solid containing 32.2 g Ba(NO3)2 per 100 g of solid. Given the balanced chemical reactions.   H₂SO4→ 2H+ + SO42-   Ba(NO3)2(s) → Ba²+ + 2(NO3-)   Ba²+ + SO4²- →Ba(SO4)(s)     Could you please explain the stoichiometric ratios involved in depth/ show a step by step process with more detail. Thanks.

Hydrogen sulfide and oxygen react to form sulfur dioxide and water, like this: 2 H, S(9)+30,(g) → 2 SO,(g)+2H,0(g9) Use this chemical equation to answer the questions in the table below. Suppose 160. mmol of H,S and None. 240. mmol of O, are added to an Some, but less than 160. mmol. empty flask. How much H,S will be O 160. mmol. in the flask at equilibrium? More than 160. mmol. None. Suppose 125. mmol of SO, and 125. mmol of H,0 are added to an O Some, but less than 125. mmol. 125. mmol. empty flask. How much SO, will be in the flask at equilibrium? O More than 125. mmol.

Assuming all gases are the same temperature and pressure how many milliliters of hydrogen gas must react to give 41.0 mL of NH3? 3H2(g)+N2(g)-->2NH3(g) Express your answer with the appropriate units. VH2=

An explosive reaction between butane and oxygen occurs as follows. 2 C4H10 (g) + 13 O2 (g) -->  8 CO2 (g) + 10 H2O (g) If 0.625 moles of butane and 3.5 moles of oxygen gas react predict the theoretical yield (in moles) of water vapor that would be produced.

Balance this unbalanced equation by entering only whole numbers into the blank. If the molar coefficient is 1, enter "1" (do not leave it blank: CaHg + O2 → CO2 + H20

Consider the following chemical reactions: KClO3 (s) ----------> KCl(s) + O2(g)  NaNO3(s) ---------> NaNO2(s) + O2(g)  5.0000 g mixture of potassium chlorate and sodium nitrate is decomposed and the mass of residuals is 3.8600 g.  The oxygen gas is collected in 359. mL. container at 25 oC by water displacement technique.  Calculate the total pressure in mmHg. the vapor pressure of H2O at 25oC is 18.3 mmHg.       K = 39.10 g/mole,   Cl = 35.45 g/mole,  Na = 22.99 g/mole,  N = 14.00 g/mole  and O = 16.00 g/mole