Consider the reaction shown: reaction    P4(s)+10cl2(g)>4Pcl5(s)+452 Kcal When 50.00 g of P4 react, ________ kcal will be ________. Group of answer choices 452; consumed 452; produced 182.4; produced 182.4; consumed 729.7; produced

Given the combustion of gasoline:  2C8H18 + 25 O2 →16CO2 +18H2O How many moles of O2 is required to react with 4.00 moles of C8H18? Select one: a. 2.00 b. 50.0 c. 25.0 d. 12.5

The actual yield can only be determined by: 8°F Mostly cloudy O Writing a balanced equation. O Calculating the theoretical yield and plugging into the percent yield. O Reviewing past reactions. O Carrying out the reaction in a laboratory. O Search H

Please balance

Classify each as exothermic or endothermic AND explain why.   N2O4(g) + 19 kcal →  2 NO2(g)      H2O(g) + CO(g) →  H2(g) + CO2(g) + 10 kcal

C6​H12​O6​ O + 6O2​  →→ 6CO2​ + 6H2​O  + Energy ​Determine the limiting reactant and how much of that limiting reactant you would need in order to use up all of the non-limiting reactant. Assume you have 25 grams of glucose and 40 grams of oxygen as reactants for the following photosynthesis reaction: A) Glucose is the limiting reactant; You would need .1388 moles of glucose to use up all of the Oxygen (non-limiting reactant).    B Glucose is the limiting reactant; You would need .208 moles of glucose to use up all of the Oxygen (non-limiting reactant).    C Oxygen is the limiting reactant; You would need 1.25 moles of Oxygen to use up all of the glucose (non-limiting reactant).    D Oxygen is the limiting reactant; You would need .8328 moles of Oxygen to use up all of the glucose (non-limiting reactant).

What is the GFM of CO₂(g)? 28.0 g/mol 44.0 g/mol 22.0 g/mol

For the following balanced equation:  CH4 + 4 Cl2 ==> CCl4 + 4 HCl Determine the number of moles of HCl that  can be made from 1.49 moles of CH4? Answer to 2 decimal places.