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A box contains a mixture of small copper spheres and small lead spheres. The total volume of both metals is measured by the displacement of water to be 432 cm^3 and the total mass is 4.32 kg. What p
In a reaction between pure acetic acid and sodium bicarbonate, 26.6 grams of sodium bicarbonate was added to 12.0 mL of acetic acid. Which reactant is the limiting reactant in this reaction?
At what temperature in degrees Celsius will your food cook in this pressure cooker set on "high"? Express your answer numerically in degrees Celsius.
cyclopropane, C3H6, is converted to its isomer propylene, CH2=CHCH3, when heated. the rate law is first order in cyclopropane, and the rate constant is 6.0x10-4/sec at 500C. if the initial concentra
Citric acid (H3C6H5O7) is a product of the fermentation of sucrose (C12H22O11) in air. Determine the mass of citric acid produced when 4.60 mol C12H22O11 is used.
An analytical chemist has determined by measurements that there are moles of magnesium in a sample of talc. How many moles of silicon are in the sample?
The molar heat capacities of iron and gold are 25.19 J/(mol * degrees C) and 25.41 J/(mol*degrees C) respectively. What is the final temperature of the water and the metals?
If 37.0 grams of hydrogen sulfide gas (H2S; MM = 34.08 g/mol) react with 37.1 grams of oxygen gas (O2, MM = 32.00 g/mol), what is the mass of sulfur dioxide (SO2, MM = 64.06 g/mol) gas produced?
If 120.9 mL of water is shaken with a gas at 0.860 atm, it will dissolve 0.00286 g of the gas. Estimate the Henry's law constant for the gas in water in units of g L-1 atm-1.
If 488 g SO2 escaped into the atmosphere and all the escaped SO2 were converted to H2SO4. How many grams of H2SO4 would be produced in the atmosphere?
The element boron has two naturally occurring isotopes with masses of 10.0129 amu and 11.0093 amu. What is the percent abundance of the second isotope?
A patient weighs 146 pounds and is to receive a drug at a dosage of 45.0 mg per kg of body weight. The drug is supplied as a solution that contains 25.0 mg of drug per mL of solution. How many mL of
A solution of sodium formate having the same molarity. How many mililiters of the Nafor solution should she add to 25 ml of the Hfor solution to make the buffer?
If a piece of aluminum with mass 3.90 g and a temperature of 99.3 degrees celcius is dropped into 10.0 cm cubed of water at 22.6 degrees celcius, what will be the final temperature of the system?
A solution of ethanol (C2H5OH) in water is prepared by dissolving 65.8 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this
Three solutions are mixed together to form a single solution. One contains 0.2 mol Pb(CH3COO)2, the second contains 0.1 mol Na2S, and the third contains 0.1 mol CaCl2. Write the net ionic equations
What would be the approximate freezing point of 0.1 molar aqueous solution of aluminium chloride at room temperature assuming complete ionisation
What volume of ammonia gas at 24°C and 753 mmHg will be produced from 4.46 g of magnesium nitride?
An 18-karat gold necklace is 75% gold by mass, 16% silver, and 9.0% copper. How many grams of copper are in the necklace? If 18-karat gold has a density of 15.5 , what is the volume in cubic centim
If the total moles of gas does not change, what is the relationship between change in enthalpy and change in internal energy?
A mixture of 82.0 g of magnesium (24.31 g/mol) and 350 g of iron(III) chloride (162.2 g/mol) is allowed to react. What mass of magnesium chloride (95.21 g/mol) can be formed?
How does the Hammond postulate explain: a.) the greater selectivity for bromination vs. chlorination of an alkane?
What type of intermolecular forces are between CH3CH2CH2Cl and cis-CHClCHCl
Given the following two solutions: 0.200 M HC2H3O2(aq) with pKa = 4.76 0.200M NaOH(aq) A mixture is made using 50.0 mL of the HC2H3O2 and 25.0 mL of the NaOH.
A 31 L tank contains a gas under a pressure of 617 atm. What volume would the gas occupy at the same temperature at 900 torr of pressure? Answer in units of L.