Chemistry, 19.05.2020 21:58, jhanellemo0112

Calculate the percent yield for the reaction above if 25.0 grams of
H2SO4 was actually produced and the theoretical yield was predicted to be 42.0 grams. (% yield = Actual/ theoretical x 100)
SO3(g) + H200 H2SO4(9)
O 59.5
O 168
O 0.595
O 1.68

Answers: 2

Show answers

Other questions on the subject: Chemistry

Chemistry, 21.06.2019 21:30, alexusjones6042

What element breaks down into yttrium-90?

Answers: 2

continue

Chemistry, 23.06.2019 05:00, mprjug6

In 1901, thomas edison invented the nickel-iron battery. the following reaction takes place in the battery. fe(s) + 2 nio(oh)(s) + 2 h2o(l) fe(oh)2(s) + 2 ni(oh)2(aq) how many mole of fe(oh)2, is produced when 4.20 mol fe and 6.70 mol nio(oh) react?

Answers: 3

continue

Chemistry, 23.06.2019 06:40, Science2019

How many joules of heat are required to raise thetemperature of 750 g of water from 11.0 °c to 19.0 °c?

Answers: 1

continue

Chemistry, 23.06.2019 08:00, oopsorry

Determine the number of moles of air present in 1.35 l at 750 torr and 17.0°c. which equation should you use? n=pv/rt what is the number of moles present? ⇒ 0.056 mol a sample of n2 gas occupying 800.0 ml at 20.0°c is chilled on ice to 0.00°c. if the pressure also drops from 1.50 atm to 1.20 atm, what is the final volume of the gas? which equation should you use? v2= p1v1t2/p2t1 what is the final volume of the gas? ⇒ 932 ml these are the answers

Answers: 1

continue

Do you know the correct answer?

Calculate the percent yield for the reaction above if 25.0 grams of
H2SO4 was actually produced...