Chemistry, 25.02.2021 01:00, ajflkasjflkasj1168
47. For each of the following unbalanced chemical equations, suppose 10.0 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected.
a. C3H2(g) + O2(g) β CO2(g) + H2O(g)
b. Al(s) + Cl2(g) β AICI3(s)
c. NaOH(s) + CO2(g) β Na2CO3(s) + H2O(1)
d. NaHCO3(s) + HCl(aq) - NaCl(aq) + H2O(l) + CO2(g)β
Answers: 2
Chemistry, 22.06.2019 08:00, anglacx5465
Why are pipes bursting in the in extremely cold weather?
Answers: 2
Chemistry, 22.06.2019 12:00, daytonalive83481
Ican determine the molar mass of an element by looking on the under the atomic mass for the element. for example the molar mass of phosphorus is 30.974 grams/mole. avogadroβs number tells me the amount of representative particles in 1 mole of any substance. this means 12.011 gram sample of carbon and a 32.0 gram sample of sulfur have the same number of atoms.
Answers: 1
Chemistry, 22.06.2019 23:50, josie311251
Be sure to answer all parts. the following equilibrium constants were determined at 1123 k: c(s) + co2(g) β 2co(g) k'p = 1.30 Γ 1014 co(g) + cl2(g) β cocl2(g) k''p = 6.00 Γ 10β3 calculate the equilibrium constant at 1123 k for the reaction: c(s) + co2(g) + 2cl2(g) β 2cocl2(g) 4.68 Γ 10 9 (enter your answer in scientific notation.) write the equilibrium constant expression, kp:
Answers: 3
47. For each of the following unbalanced chemical equations, suppose 10.0 g of each reactant is take...
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