14.7 g of nitrogen gas is combined with 4.1 g of oxygen gas. 2.125 g of nitrous oxide (nitrogen monoxide) is formed during the experiment. What is the percent yield? (Hint: write the balanced equation and find the limiting reagent) M (O) = 16 g/mol; M (N) = 14 g/mol Answer: Percent yield(%)=

One night you and your friend decided to help in agriculture. The farmer you are helping reacted 90 Kg of Calcium fluoride phosphate (Cas(PO4)3F) and 30L of sulfuric acid(H2SO4), so far he has collected 5Kg of hydrofluoric acid (HF) and the farmer wants to know the % yield of the HF to estimate the time needed to complete the reaction. Balance the equation, calculate the molecular weight and mols of Cas(PO4)3F and H2SO4 (Density of Sulfuric acid 1.84 g/cm3), Calculate the limiting reagent, the percent yield of HF and the number of molecules of so far. If the density of HF is 1.15 g/cm3 and the temperature of the 10 L vessel HF is contained is 25 C what is the pressure of the contained in which HF is collected? Ca(H2 PO4)2 (aq) + CaSO4 (aq) + HF (g) Cas(PO4)3F (s)+H2SO4 (aq)

What is the % yield of the reaction? What is the limiting reagent? Show complete calculations for the theoretical and % yield calculations, please. Bromobenzene: 4.5mL Magnesium:1.0g Methyl benzoate:2.5mL

0 A reaction of 36.9 g of Na and 46.9 g of Br₂ yields 51.9 g of NaBr. What is the percent yield? 2 Na(s) + Br₂(g) - ->> 2 NaBr(s) percent yield:

A) Determine the molecular formula of X (the starting reagent)  B) Write a balanced equation for this reaction C) Determine the theoretical mass of the CO2 produced if 0.2 mol of O2 is completely consumed D) If the combustion reaction produced is 3.0g of CO2, determine its percentage yield

For the following reaction, 5.86 grams of carbon tetrachloride are mixed with excess methane (CH4). The reaction yields 5.93 grams of dichloromethane (CH2CI2). What is the percent yield of this reaction? CH4 + CCh --> 2CH2Cl2 27.6% 109.1% 91.65% 84.5%

H3PO4 + 3NaOH ---> Na3PO4 + 3H2O     If you mix 100 ml of 8.5M H3PO4 with 150 ml of 9.0M NaOH, how many g of Na3PO4 will be produced? What is your limiting reagent? If you only got 59.5 g of Na3PO4, what is your percent yield? How many grams of your excess reagent do you have left over?

Find the mmol for all 4 compounds then find all 3 yields. Indicate the limiting reactant with an asterisk. (The product is 2.809 grams)

When 12.0 g of carbon is burned in oxygen during an experiment, only 39.3 g of carbon dioxide was collected. What is the percentage yield?   C + O2 -> CO2   Answer in standard notation, rounded to the nearest tenth of a percent.

Give the percent yield when 28.16 g of CO 2 are formed from the reaction of 3.000 moles of C 8H 18 with 6.000 moles of O 2.  2 C 8H 18 + 25 O 2  → 16 CO 2 + 18 H 2O     26.67%     33.33%     75.00     16.67%     66.67%