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1. Liquid ethyl alcohol at 77.0°F is burned in 100.% theoretical air. Determine the heat produced per kgmole of fuel when the products are at 540.°F. The molar specific enthalpy of formation of this fuel is -277:69 MJ/kgmole:
2. Methane gas (CH4) at -60.0°C is burned during a severe winter with 200.% theoretical air at the same temperature. The products of combustion are at 300.°C. Assuming constant specific heats, find the heat released per kgmole of fuel.
Calculate the amounts of Cu AND Br2 produced in 1.0 h at inert electrodes in a solution of CuBr2 by a current of 4.50 A. MW (Cu) = 63.55 g/mol /MW (Br2) = 160 g/mol & n = 2 mol e-
How many resonance structures does HSO4- have. The way I've been doing it would make it 12 but that seems like it'd be too many.
If 1.50 g of X reacts with 3.54 g of M to produce 4.22 g of a compound with the formula M4X3, and the atomic mass of M is 48.5 amu.
Given Data; P4+6Cl2=4PCl3 change temp= -2439 kj ,4PCl5=P4+10Cl2 change temp= 3438 kj calculate change in temp for the reaction PCl5=PCl3+Cl2.
The house is losing heat to the outside air through the walls and windows at a rate of 60,000 kJ/hr while the energy generated within the house from people, lights,and appliances amounts to 4,000 kJ/hr.
What is the most significant intermolecular attraction in a pure sample of CH3F
When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 16.8g of carbon were burned in the presence of 57.4g of oxygen, 12.6g of oxygen remained unreacted. What mass of carbon dioxide was produced
Provide a balanced equation for the oxidation of the following: 2-propanol to acetone by means of Cr2O7-2/H+. Please show all steps to obtain the final balanced equation.
If 250.0 mL of 0.354 M Phosphoric acid need to be prepared, how many grams of H3PO4 need to be added to water to make this solution
Explain why in some cases a compound may be an acid as well as in other case not? For example, HCL (hydrogen chloride).
A buffer solution contains acetic acid (HC2H3O2) at a concentration of 1.15 M and sodium acetate (NaC2H3O2) at a concentration of 2.05 * 10 to -2 M. The value of Ka for acetic acid is 1.75 * 10 to -5. Calculate the pH of this solution using the He..
The pH of a bicarbonate-carbonic acid buffer is 7.80. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3-).
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