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A 4.20 g fuel with unknown heating value is burned in a calorimeter. The calorimeter has a constant of 15.0 J/K. Initially, the temperature is 25.0 degC and the temperature increased by 5.42 K.
What is the final temperature of the calorimeter? in degC
A 4.20 g fuel with unknown heating value is burned in a calorimeter. The calorimeter has a constant of 15.0 J/K. Initially, the temperature is 25.0 degC and the temperature increased by 5.42 K.
What is the delta T of the calorimeter? in degC
Calcium reacts with water to produce hydrogen gas and aqueous calcium hydroxide. (a) Write the balanced equation for the reaction. (b) How many mL of water (d= 1.00 g/mL) are required to produce 7.00 L of dry hydrogen gas at 1.05 atm and 32°C?
Nitrogen oxide is a pollutant commonly found in smokestack emissions. One way to remove it is to react it with ammonia. (a)Write the balanced equation for this reaction and (b) calculate how many liters of ammonia are required to change 12.8 L of nitrogen oxide to nitrogen gas? Assume 100% yield and that all gases are measured at the same temperature and pressure (STP).
7.45g KCl is dissolved in 50 mL water. Calculate the concentration of KCl in terms of molarity, molality and normality.
Define electron affinity citing its trend of variation along the periodic table.
Why do the nails corrode at points of stress? Can you tell where the stress points are? What is the cause of the stress?
A student weighs out a 1.91 g sample of NH4CH3COO , transfers it to a 100. mL volumetric flask, adds enough water to dissolve it and then adds water to the 100. mL tick mark.
What is the molarity of ammonium acetate in the resulting solution?
Calculate the mass in grams of NaOH that must be added to make a 15% solution. Density of water= 1g/ml.
The following data apply to the reaction:
A(g) + 3B(g) + 2C(g) → products.
Rate[A][B][C]X0.200.400.108X0.400.400.20X0.200.200.204X0.400.400.10
Determine the rate law for the reaction.
