A. 1.
There are 7 O on left and 6 O on right. So to balance it out write two as coefficient of H2O.
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of H4As2O7 and As2O5.
This is the balanced chemical equation. As one reactant (H4As2O7) breaks down to form two products (As2O5 and H2O) so it is a decomposition reaction.
2.
There are 2 O on left and 1 O on right. So to balance it out write two as coefficient of N2O.
There are 2 N on left and 4 N on right, so to balance it out write 2 as coefficient of N2
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of O2.
This is the balanced chemical equation. As two reactants (N2 and O2) combine to form one product (N2O) so it is a combination reaction.
3.
There are 2 Br on left and 1 Br on right. Also there are 2 I on right and one on left. So to balance these out write two as coefficient of NaI and NaBr.
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of I2 and Br2.
This is the balanced chemical equation. As one reactive element (Br2 in this case) replaces the less reactive element (I2 in this case) from its compound (NaI in this case), so this is a single replacement reaction.
4.
There are 2 H on right and 1 H on left. There are 2 NO3 groups on right and one on left. So to balance these out write two as coefficient of HNO3.
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of PbCrO4 and H2CrO4.
This is the balanced chemical equation. As there is a mutual exchange of ions between the two reacting compounds to from two new compounds this is a double replacement reaction.
5.
There are 3 C on left and one on right. So to balance it out write three as coefficient of CO2.
There are 8 H on left and 2 on right so to balance it out write 4 as coefficient of H2O.
Now there are 3x2+4=6+4=10 O on right and 2 O on left. So to balance it out write 5 as coefficient of O2
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of C3H8
This is the balanced chemical equation. As in this reaction a hydrocarbon (C3H8) reacts with oxygen (O2) to form CO2 and H2O, this is a combustion reaction.
6.
There are 4 Cl on left and 2 Cl on right. So to balance it out write two as coefficient of MgCl2.
There are 2 Mg on right and one on left, so to balance it out write 2 as coefficient of Mg.
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of TiCl4 and Ti.
This is the balanced chemical equation. As one reactive element (Mg in this case) replaces the less reactive element (Ti in this case) from its compound (TiCl4 in this case), so this is a single replacement reaction.
7.
There are 2 CN on right and 1 on left. So to balance it out write two as coefficient of KCN.
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of CuSO4 and K2SO4.
This is the balanced chemical equation. As there is a mutual exchange of ions between the two reacting compounds to from two new compounds this is a double replacement reaction.
8.
There are 3x2=6 O on left and 2 O on right. So to balance it out write three as coefficient of O2.
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of Ca(ClO3)2 and CaCl2.
This is the balanced chemical equation. As one reactant (Ca(ClO3)2) breaks down to form two products (CaCl2 and O2) so it is a decomposition reaction.
9.
There are 2 Na on left and 1 O on right. So to balance it out write two as coefficient of NaOH.
Now we can see that all the atoms are balanced in this reaction. Write 1 as coefficient of Na2O and H2O.
This is the balanced chemical equation. As two reactants (Na2O and H2O) combine to form one product (NaOH) so it is a combination reaction.
10.
There are 6 C on left and one on right. So to balance it out write six as coefficient of CO2.
There are 14 H on left and 2 on right so to balance it out write 7 as coefficient of H2O.
Now there are 6x2+7=12+7=19 O on right and 2 O on left. So to balance it out write 19/2 as coefficient of O2
Multiply the whole equation by two
Now we can see that all the atoms are balanced in this reaction.
This is the balanced chemical equation. As in this reaction a hydrocarbon (C6H14) reacts with oxygen (O2) to form CO2 and H2O, this is a combustion reaction.
A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a...
D. Complete the following stoichiometry problems. Show ALL of your work to receive full credit. Equations and mole-to-mole relationships 21. For the following reaction: 4Cr(s) + 302(g) → 2Cr2O3(s) a. How many moles of oxygen (O2) would react with 0.35 moles of chromium (Cr)? b. Starting with 10.4g of Oz, how many moles of Cr203 can be produced: c. How many grams of Cr metal would be needed to produce 38.2g of chromium (III) oxide? 22. Sulfuric acid (H2SO4) is...
B. Complete the following equations by writing the formula(s) of the product(s) and balancing the equation with coefficients. Type of Reaction Balanced Equation Single Replacement 11 Zn + H2SO4 Double Replacement 12 _AgNO3 ВаCl2 + 5 C4H10 13 O2 Combustion 14. HgO Decomposition Al Cl2- Combination 15 C. Write the balanced chemical equation for the following chemical reactions. Include the correct formulas for all reactants and products and balance with coefficients. Identify the type of reaction in the right column....
--xal Yield and Percent Yield combusts with oxygen to form carbon dioxide and water by the following reaction: pentane combud CsHız(l) + 8 O2(g) → 5 CO2(g) + 6 H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: compare it to either of the products). b. What is the theoretical yield (in grams) of carbon dioxide and water for this reaction? Hydrogen reacts with nitrogen to form ammonia by...
The combustion of pentane can be represented by the following equation: __C5H12 (g) + __O2(g) → __CO2(g) + __H2O(g) Balance the equation and answer the next three questions. 1. If 270. g of C5H12 and 970. g O2 react, which reactant is used up first? (enter pentane or oxygen) 2. What is the mass of carbon dioxide produced? (Give your answer to 3 sig figs.) grams 3. What is the mass of water produced?(Give your answer to 3 sig figs.)...
Name FUL L U Stoichiometry worksheet (Lab) Please complete the following problems during lab. Do all of your work on a separate sheet of paper. Show all of your work for full credit and circle your final answer. 1) How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation? C3H8 (8) +502 (8) ► 3002 (8) + 4H20 (8) 2) In the reaction 2 C(s) + O2(g) 66.0 g of carbon monoxide?...
27) When propane (C3H8) reacts with oxygen, carbon dioxide and water are produced. The balanced equation for this reaction is: C3H8 (g) + 5O2 (g) ---> 3CO2 (g) + 4H2O (g) Suppose 17.8 moles of oxygen react. The reaction consumes ___ moles of propane (C3H8). The reaction produces ___ moles of carbon dioxide and ___ moles of water. How many grams of water are produced in the complete reaction of 27.2 grams of propane (C3H8)? ___ grams
4. HgO → Combustion 15. Decomposition Al +_ Cl2 → Combination c. Write the balanced chemical equation for the following chemical reactions. Inclu formulas for all reactants and products and balance with coefficients. Identity in the right column. 1 coefficients. Identify the type of reaction Balanced Equation Type of Reaction 16. Iron and oxygen react to form iron (III) oxide. 17. Silver nitrate and magnesium chloride react to form may rate and magnesium chloride react to form magnesium nitrate and...
Problem 9.7 Heats of Reaction Use tabulated heats of formation to determine the standard heats of the following reactions in kj, letting the stoichiometric coefficent of the first reactant in each reaction equal one. Physical Property Tables Oxidation of Nitrogen Nitrogen (N2) and oxygen (O2) react to form nitrogen tetraoxide. AH, kJ the tolerance is +/-2% Oxidation of Alkanes Gaseous n-pentane + oxygen react to form carbon monoxide + liquid water. ΔΗ) = kJ the tolerance is +/-2% Oxidation of...
Write and balance the following chemical equations. Iron (III) oxide reacts with carbon monoxide to yield iron and carbon dioxide. Rubidium reacts with water to yield rubidium hydroxide and hydrogen. Copper (II) chloride reacts with ammonium phosphate to yield ammonium chloride and copper (II) phosphate. Ammonia and oxygen react to form nitrous oxide (also known as nitrogen monoxide) and water.
Limiting Reactant, Theoretical Yield and Percent Yield 2. Pentane combusts with en to form carbon dioxide and water by the following reaction: CsHız(1) + 8 O2(g) → 5 CO2(g) + 6H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxy compare it to either of the products). he is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: b. What is the theoretical yield (in grams) of carbon dioxide and water for this...