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Hydrogen peroxide decomposes into water and oxygen gas. how many moles of hydrogen peroxide are needed to produce 1.5 mol of oxygen (balenced equation needed)
Moles of hydrogen peroxide needed=1.5 moles
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The mass of an empty container is 93g the mass of the container filled with water is 119g what is the volume of the container? the density of water is 1g/cm^3 answer in terms of cm^3
119-93 = 26V = Mass/density= 26/1= 26ml
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Flourine gas is in a 5.0 L container that is 25 C and 2 atm. A certain amount of hydrogen with a partial pressure of .5 is added to the container. What is the mole ratio of hydrogen?
total pressure is 2 atmFlourine+.5 atmHydrogen=2.5 atmtotalremember that pH/ptot=nH/ntot=vh/vtot so the mole ratio of hydrogen to the mixture is is .5/2.5=.2 molHydrogen to 1 moltotal
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Zinc and HCl react to form ZnCl2 and hydrogen gas. How many grams of H2 can be produced if 4.25g of Zinc react with 25 mL of 3.00M HCl?
25 mL x (1L/1000 mL) x (4 mol HCl/1L) x (1 mol Zn/2 mol HCl) x (65.38 g Zn/1 mol Zn) = 3.269g = ~ 3.3g of ZnParts explained25 mL...
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what term in chemistry refers to a gas held in a closed container on top of a solid or liquid phase?
Pressure of gas
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a sample oh hydrogen gas, H2(g), is placed in a 0.500L container at 295 K. The gas pressure is 1.442bar. how many moles of H2 gas are in the container
pV=nRTT = 295 KV = 0.5 L = 0.5*10-3 m3p = 1.442 bar = 144200 Pa R = 8.314 J/mol*Kn = pV/RT = (144200*0.5*10-3)/(8.314*295) = 0,029 mol.
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A 2.83 L container of oxygen gas at 25.2 °C is heated to 46.8 °C. Assuming that the volume of the container can vary, what is the new volume of the gas
V2 = 3.035 L
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Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.08 mol of NH3 6.32 mol of O2 react
4NH3+5O2---->4NO+6H2O2.08 moles of ammonia will require 2.6 moles of oxygen gass from the mole ratio of 4:5 the ratio of ammonia to oxygen.(2.08÷4)×5=2.6This implies that ammonia is the limiting reagent...
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The reaction N2(g) + 2O2(g) ! N2O4(g) occurs in a closed
container. If 8.0 moles N2(g) are made to react with 12.0 moles
O2, the limiting reagent and the theoretical yield of N2O4 are:
Solution:According to the reaction equation for 1 mol of N2 are needs 2 moles of O2.Therefore, for 8.0 moles N2 are needs 16 moles O2.The limiting reagent is O2.The theoretical...
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when nitrogen gas reacts with hydrogen gas,ammonia gas is formed.How many grams of hydrogen gas are required to react completely with 3,5 L of nitrogen at STP?
Solution:A chemical equation must be balanced:N2 + 3H2 = 2NH3According to the reaction equation for 3 mol of H2 is needed 1 moles of N2.Therefore, mass of H2 = V...
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