(24) SEP Apply Mathematical Concepts The incomplete combustion of ethene is given by the equation C2H4(g) + 2O2(g) → 2CO(g) + 2H20(g). Cenene is given by the equation C.H.(g) + 20,(g) → 2CO(g) + 2H2O(g). If 2.70 mol C,H, is reacted with 6.30 mol O a. identify the limiting reagent. b. calculate the moles of water produced.

(6)For the following balanced reaction use the mass of the chemical provided to solve the mass of the chemical asked for.  6 CO2 +  6 H2O  -->  1 C6H12O6   +   6 O2   202 g of CO2 is consumed by a plant undertaking this photosynthesis reaction.  Find the mass of C6H12O6 produced.

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Consider the combustion reaction of a hydrocarbon compound here: C2H4(g) + 302(g): 2 CO2(g) + 2 H20(g) ----> When 5.00 mol of C2H4 and 12.0 mol of O2 are added to the reactor, How many moles of CO2 can be produced by the reaction? O 4.00 mol of CO2 O 10.0 mol of CO2 O 5.00 mol of CO2 O 8.00 mol of CO2

Silicon tetrachloride (SICI4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2C12(g) -> SiCl2(1) In one reaction, 0.507 mole of SiCI4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SICI4 = 169.9 g/mol; MW CI = 35.453 g/mol (A) 36 grams (B) 72 grams 27 grams D) 63 grams

The enthalpy for combustion for ethanol is -1370.7 kJ/mole and occurs via the following balance chemical reaction.   C2H6O (l)         +          3 O2 (g)           -->        2 CO2 (g)         +          3 H2O (g)   If 0.461 grams of ethanol are combusted in the presence of 1.28 g of O2, answer the following.   a. How many grams of CO2 could be produced?   b. How much heat is released?   c. What is the change in internal energy (DU)?

Silicon tetrachloride (SiCl4 ) can be prepared by heating Si in chlorine gas:  Si(s) + 2Cl2(g) -> SiCl4(l) In one reaction, 0.507 mole of SiCl4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SiCl4 = 169.9 g/mol; MW Cl = 35.453 g/mol   63 grams   27 grams   72 grams   36 grams

6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles

Consider the following reactions:CoO (s) + CO (g) D CO2 (g) + Co (s) Kc(1) = 490.2 CoO (s) + 2 H2 (g) D 2 Co (s) + 2 H2O (g) Kc(2) = 4.5 x 103a. Write the overall equation for the reaction of hydrogen gas and carbon dioxide gas to produce carbon monoxide gas and steam.

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH₂ (g) + 20₂(g) → HNO3(g) + H₂O (g) Suppose the yield of the first step is 61.% and the yield of the second step is 77.%. Calculate the mass of nitrogen required to make 10.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 Explanation Check. ☐ x10 8 X 09 0.0 S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |