The reaction of phosphine with oxygen has the following
unbalanced
equation
PH3 + O2 → P4O10 + H2O
The coefficient for oxygen in the balanced equation is...
Hint: Balance the reaction on a sheet of scratch paper before attempting to answer this question.
First of all balance phosphorus by multiplying 4 with PH3
4PH3 + O2 ------> P4O10 + H2O
Now balance hydrogen by multiplying 6 with H2O
4PH3 + O2 ------> P4O10 + 6H2O
Now balance Oxygen by multiplying 8 with O2
4PH3 + 8O2 -------> P4O10 + 6H2O
the coefficient for oxygen in the balanced equation is 8
The reaction of phosphine with oxygen has the following unbalanced equation PH3 + O2 → P4O10...
The reaction of hydrazine with dinitrogen tetroxide has the following unbalanced equation N2H4 + N2O4 N2 + H2O The coefficient for nitrogen gas in the balanced equation is...
On scratch paper, balance the following redox reaction in basic solution, and then answer the question below. MnO4- + I- -> MnO2(s) + I2 (basic) When the equation, is correctly balanced, what is the coefficient in front of I2? a. 1 b. 2 c. 3 d. 6 e. 12 On scratch paper, balance the following redox reaction in basic solution, and then answer the question below. BrO3- + Cr(OH)3(s) -> Br- + CrO42- (basic) When the equation, is correctly balanced,...
The unbalanced equation for the reaction between
hydrogen sulfide and oxygen gas
is shown below.
Balance the equation (enter the smallest integer possible in
each box, including the integer "1" when needed) and determine the
amount of O2 consumed and the amounts
of H2O and
SO2 produced when
0.970 mol of H2S
reacts.
consider the unbalanced equation for the following reaction
O2(g) + C3H8
Reviewing Pool 4 Question 1 Available Point 10 Consider the unbalanced equation for the following reaction Oxg) -CH() - COX). How Determine the amount of H2O(l) formed in the reaction if 9.50 moles of OC reacts with an excess of C ) and the percent yield of Ho %
Consider the unbalanced equation for the following reaction: O2(g) + C6H5COOH(aq) → CO2(g) + H2O(l) If 54.0 grams of C6H5COOH(aq) reacts with an excess of O2(g) and 103. grams of CO2(g) is formed, determine the percent yield of CO2(g). (the answer is 76.0%, I want to know the process)
Use the unbalanced equation C2H6O + O2 → CO2 + H2O to answer the following questions. If 2 mol of C2H6O and 4 mol of O2 are reacted, the limiting reactant is __________. A. O2 B. C2H6O C. C2H6O and O2 are in the correct ratio D. There is not enough information given to answer the question.
When a mixture of 13.0 g of acetylene (C2H2) and 13.0 g of oxygen (O2) is ignited, the resultant combustion reaction produces CO2 and H20. The unbalanced equation for this reaction is shown below. C2H2 + O2 CO2 + H2O Part A Write the coefficients in the balanced equation in the order the substances are written. Templates Symbols undo rédo reset keyboard shortcuts 'help ΑΣ και C2H2, O2, CO2, H2O Submit Request Answer Part B Which is the limiting reactant?...
Oxygen reacts with sulfur in the following unbalanced reaction: S8 (s) + O2 (g) ⟶ SO3 (g) unballanced How many grams of sulfur would be required to react with 80.0 L of oxygen gas at STP?
PLEASE ANSWER EACH QUESTION OR DO NOT ANSWER AT ALL. THANK
YOU!
4. Consider the following unbalanced net redox equation: HCI + KMnO, (aq) + H,02 (aq) -. MnC12 (aq) + O2 (g) + KCI in an acid solution a. Determine the oxidation state of each atom or ion in the above reaction: b. Which atom is being oxidized? Which atom is being reduced? C. Which species is the reducing agent? Which is the oxidizing agent? d. Write the net...
Acetylene gas produced in the experiment in question #2 is the gas used in welding torches. Recall its formula is two carbons and two hydrogens. You could take the balloon full of acetylene from question #2 and tie it to the end of a meter stick. Then if you hold the balloon near a burner flame, the balloon will explode as the oxygen from the air (O2) combines with the acetylene (two carbons and two hydrogens). The exothermic reaction produces...