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How many moles of Na3C6H5O7 can be produced if one tablet containing 0.0119 mol of NaHCO3 is dissolved?
how to calculate the enthalpy of air at -80 degree centigrade temp and -161 degree centigrade at 37 barg and 4 barg respectively.
535 g piece of copper tubing is heated to 91.5°C and placed in an insulated vessel containing 58.5 g of water at 29.5°C. Assuming no loss of water and heat capacity for the vessel of 10.0 J/K,
h2s and h2o have similar structures and their central atoms belond to the same group. why is h2s a gas at room temperature and h2o a liquid? explain using principles of bonding.
Compounds and predict their relative C=O vibrational frequencies based on the importance of the contributing resonance structures. List in them order from highest to lowest frequency.
calculate the pH of solution formed by mixing 150 mL of 0.10M HC7H5O2 with 100 mL of 0.30M NaC7H5O2. The Ka for HC7H5O2 is 6.5 E -5
Calculate the mass of silver chloride and dihydrogen monosulfide (H2S) formed when 85.6g of silver sulfide reacts with excess hydrochloric acid.
IF 4.50 mole of ethane undergo combustion according to the unbalanced equation C2H6+O2=CO2+H2O how many moles of oxygen are required?
A tanker truck carrying 5.0 x 103 kg of concentrated sulfuric acid (H2SO4) tips over and spills its load. If the solution is 95% sulfuric acid by mass and has a density of 1.84 g/L how many kilogram
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.050 M, [H2] = 0.045 M, [
The vapor pressure of water at 29 is 30.0 . How many moles of can be produced from grams of in magnesium-aluminum alloy? The molar mass of is 24.31.
The naturally occurring compound urea, CO(NH2)2, was first synthesized by Friedrich Wohler in Germany in 1828 by heating ammonium cyanate. This synthesis was a significant event because it was the f
In the reaction where the potassium chlorate is decomposed into potassium chloride and oxygen. How much oxygen can be made from 45.8g of the potassium chlorate?
How much will the temperature change when 730 g of each of the following materials absorbs 1240 cal of heat energy?
Calculate the theoretical yield of when 110g of C2H6 reacts with 207g Cl2 of , assuming that and react only to form C2H5Cl and HCl . Calculate the percent yield of if the reaction produces 169g of C
When 9.6 grams of NaBr are dissolved in enough water to create a 165-gram solution, what is the solution's concentration, expressed as a percent by mass?
What is the half reaction showing the reduction of dichromate ion? and what is the half reaction showing the oxidation of iron (II) ion?
A calorimeter containing 200.0 mL of water was calibrated by carrying out a reaction which released 15.6 kJ of heat. If the temperature rose 3.25 degrees celcius then the heat capacity of the calori
How much heat (in Joules) is gained by the water where a chemical reaction takes place in 100 mL aqueous solution and has a temperature increase of 14C?
The active ingredient in toothpaste is sodium fluoride, an anticavity agent. a 170 g tube of toothpaste lists the concentration of sodium fluoride a s0.24%. how many grams of sodium fluoride are in
a sample of helium gas initially at 37 degrees celsius, 785 torr and 2.00L was heated to 58.0 degrees celcius while the volume expanded to 3.24L. What is the final pressure in atm.
A solution of I2 was standardized with ascorbic acid. Using a 0.1137-g sample of pure ascorbic acid, 26.75 mL of I2 were required to reach the starch end point. What is the tiger of the iodine solu
A solution of 11.3g of electrolyte in .105 kg of water freezes at -2.36 degree centigrate at standard temperature. what is the molecular weight , in gram per mole, of this compound. kf =1.86
A sealed container contains 6 mol of hydrogen and 1 moles of nitrogen gas. If the total pressure in the container is 1.5 atm, what is the amount of pressure exerted by the hydrogen?
The sales of 'Gourmet Popcorn' seems to be losing market share and a number of seemingly unknown brands are creating serious competition. Please, conduct the following research.