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A chemist dissolves 0.9 g of an unknown monoprotic (one acidic H) acid in water. She finds that 14.6 mL of 0.426 M NaOH are required to neutralize the acid. a. How many grams of acid are present?b. How many moles of base are required to reach the equivalence point?c. How many moles of acid are present initially?d. What is the molar mass of the acid?e. What is the chemical formula and name of this acid?
The average person generates about 2500 Kcal of heat a day. How many kilowatt-hours of energy is this? If walking briskly dissipates energy at 500 W, what fraction of the day's energy does walking one hour represent.
A graduated cylinder contains 25.0 of water. What is the new water level after 34.2 of silver metal with a density of 10.5 is submerged in the water.
Determine the numbers of moles of iron that would be formed from 6.2 moles of CO (carbon monoxide) combining with excess of iron (III) oxide (Fe2O 3 )?
Determine which metal will reach the lowest temperature If the same amount of heat is added to both the metals?
Calculate the specific heat was? Would your computed specific heat be , too low, too high or not affected if you had not dried the metal before placing it into the Styrofoam cup. Explain your answer?
Determine the volume of 0.M baryta (Barium hydroxide is the chemical compound with the formula Ba(OH) 2 ) that is needed to neutralize 35 ml of 0.2M phosphoric acid (H 3 PO 4 ), ?
What liquid is insoluble in water and soluble in cyclohexane and alcohol; and has a boiling pint of 58 degress Celsius at 670 mm Hg.
Compute the boiling point of this solution if Kf and Kb for H 2 O are given as 1.86°C/m and 0.512 °C/m , respectively.
Determine delta H of this reaction (kJ/mol H 2 SO 4 ) - When 24.4 mL of 0.500M sulphuric acid ,H 2 SO 4 is combined to 24.4ml of 1.00M potassium hydroxide KOH in a coffee cup calorimeter
The density of chloroform, a widely used organic solvent, is 1.4832 at 20 . How many milliliters would you use if you wanted 119.0 of chloroform.
When relatively small amounts of magnesium burns, the fires are extinguished using commercially available dry powder. Why might this fire rekindle days later as someone tries to remove the residue with water?
Calculate the equilibrium constant for each of the reactions at 25 ° C .O 2 (g)+2H 2 O(l)+2Cu(s)→4OH - (aq)+2Cu 2+ (aq) Express your answer using one significant figure.
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