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While 1.00g of compound X is combusted in a bomb calorimeter which contains 2100g of water, the temperature increases from 10.000C to 23.630c. The calorimeter (excluding the water) has a heat capacity of 510J/K. Compute the molar heat of combustion for compound X (Mx = 90.00g/mol).
The critical constants of ethane are Pc= 48.20 atm, Vc= 148 cm3mol-1, and Tc= 305.4 K. Calculate the van der Waals parameters of the gas and estimate the radius of the molecules.
Write a chemical reaction equation that shows what happens when HNO3 is added to MnCO3. Remember to include the physical state symbols.
A 20.00 mL solution of nitric acid, HNO3, required 25.7 mL of 0.1313 M NaOH to reach a bromthymol blue end point. What is the concentration of the nitric acid solution
Could you tell me what is the purpose of this reaction (Michael and aldol condensation reactions), and the stepwise mechanism of the reaction.
According to Raoult's law, which statement is false?
The pH of the solution when exactly 13mL of base has been added was 3.82. You notice that the concentration of the unknown acid was 1.0M. What are the Ka and the pKa of your unknown acid
What mass of copper nitrate would be produced from the complete reaction of 45.6 g of copper, according to the chemical reaction shown below? Cu + 2 AgNO_3 ----> Cu(NO_3)_2 + 2 Ag
Someone is forced to titrate a solution containing 100 mL of .250M sodium acetate with .125 M nitric acid. Calculate the pH of the solution after adding 50.0 mL of the nitric acid.
Write the formula and calculate the molar mass of KHP (KHP is not potassium hydrogen phosphorus). Q2 When conducting this experiment, why is it necessary to standardize your NaOH solution before titrating your unknown acid?
What hybridization would you expect for the indicated (bold) atom in each of the following molecules?
Describe the effect on pH (increase, decrease, or no change) that results from each of the following additions: (a) potassium acetate to an acetic acid solution,
An unknown metal hypochlorite salt, M(ClO)2, is subjected to analysis by iodometric titration: the salt is dissolved in dilute sulfuric acid, treated with excess aqueous KI, and then titrated with Na2S2O2 in the same manner as in your experiment
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