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1. What's the mass of sodium oxide produced if 1.5 g of sodium reacts with excess gaseous oxygen? (Write the balanced equation.)
2. Hydrochloric acid reacts with aluminium to form aluminium chloride and gaseous hydrogen. What's the mass of aluminium required to produce 1.0 kg of aluminium chloride if there is excess acid?
3. 2KMnO4 + 5H2SO3 ? K2SO4 + 2MnSO4 + 2H2SO4 + 3H2O
Calculate the mass of:
a. sulphurous acid, H2SO3, required to react with 3.16 g of potassium permanganate, KMnO4
b. manganese (II) sulphate produced when 5.65 g of potassium permanganate react with excess sulphurous acid
c. potassium permanganate required to produce 5.00 g of manganese (II) sulphate.
4. Calculate the mass of 80% pure aluminium required to produce 9.65 kg of aluminium oxide.
How many liter of ethane, measured at 15 degrees C and 711 torr, must be burned to liberate 2.73 * 10^4 KJ of heat? 2(C2H6) +7(O2) ----> 4(CO2) + 6(H2O) [delta H= -3.12 *10^3]
Assume that gasoline is burned with 99% efficiency in a car engine, with 1% remaining unburned in the exhaust gases as VOCs. If the engine exhausts 16 kg of gases (MW = 30) for each kg of gasoline (MW = 100), calculate the fraction of VOCs in the ..
An analytical procedure requires a solution of chloride ions. how many grams of caCl2 must be dissolved to make 2.15 L of 0.0520 M Cl-.
a 1.30 m solution of citric acid h3c6h5o7 in water has a density of 1.10 gcm3. calculate the mass percent molality mole
What is the magnitude of the change in pH when 1.8 g of NaOH is added to 1.00 L of a solution that is0.100 M in NH4Cl
A 4.369 g sample of metal is placed in a flask. Water is added to the flask and the total volume in the flask is read to be 126.4 ml. The mass of the water
93.0 ml of 0.150 m magnesium hydroxide is added to 57.0 ml of 0.4 m nitric acid. magnesium nitrate and water are
when 56.6g of calcium and 30.5g of nitrogen gas underfo a reaction that has a 93.0% yield, what mass g of calcium nitride forms.
During the dehydration reaction when acetaldehyde was reacted with KOH in ether, an intermediate was formed. What was this intermediate that was eventually converted to the final product?
What is the concentration of chromium ion present in a 0.01976 M solution of potassium hydroxide in contact with a large excess
In the titration of a solution of the extremely weak acid, HCN (Ka = 6.2 x 10-10), by a solution of sodium hydroxide of equal concentration,
What is the predominant form of Ile at pH 6 (assuming the pKa of the carboxylate is 3 and the amino group is 9?
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