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1. Why must you avoid using your hands in handling the magnesium ribbon and the crucible and cover? 2.Why must objects be cooled to room temperature before taking their weights(masses)? 3. At the high temperatures used in this experiment, some of the magnesium reacts with nitrogen gas in the air forming magnesium nitride, Mg3N2. Write the balanced equation for this reaction. 4. If 6.0 of MG is heated at high temperatures and is completely converted to magnesium nitride as in the equation above, how grams of magnesium nitride will be formed?
Which of the following describes the best way to prepare 500. mL of a 0.20 M solution of benzene (C6H6?)?(78.11 g /?mol) dissolved in carbon tetrachloride (CCl4?)?(153.82 g /?mol).
To a sample of alkaline earth metal carbonate (MCO3; 0.250 g) was added 30.0 mL HCl (0.250 mL). Carbon dioxide gas evolved out from the solution. After the reaction was completed.
When a ketone is treated with LiAlH4 followed by addition of water, what general class of product results?
If each bottle contains 0.358 pint of mouthwash with a density of 0.880g/mL , how many kilograms of alcohol are in 200 bottles of the mouthwash.
A mixture of helium and neon gases is collected over water at 28.0 C and 745 mmHg. if the partial pressure of helium is 368 mmHg, what is the partial pressure of neon?
For 220.0 mL of a buffer solution that is 0.205 M HCHO2 and 0.295 M KCHO2, calculate the initial and the final pH after adding 0.010 mol of NaOH.
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.
a sample of ammonia gas at 1.2 atm compressess from 500 ml to 250 ml. if the temerature remains constant, what is the new pressure of the gas? what formulas were used?
Find the heat of combustion in kJ/g for each gas. These values are valid at 25°C, where the water produced by the reaction is in the liquid state.
Determine the numerical values of the parameters A, B, and C in the Antoine equation relating vapor pressure of pure substances to temperature using an appropriate linear regression procedure.
The elements X and Y form a compound that is 33.33% X and 66.67% Y by mass. The atomic mass of X is twice that of Y.What is the empirical formula of the compound?
A 184-mg sample of Na2CO3 is dissolved in H2O to give 3.00L of solution. What is the concentration of Na+ in parts per million (ppm)?
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