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A 350.0 g sample of copper is initially at 25.0 °C. It absorbs 12.50 kJ of heat from its surroundings. What is its final temperature, to the nearest tenth of a degree?
Consider the reaction CaCN2 + 3 H2O → CaCO3 + 2 NH3 . How much CaCO3 is produced if 47.5 moles NH3 are produced
What is the boiling point of a mixture composed of 95.0 g HOCH2CH2OH (ethylene glycol) and 205 g H2O? The boiling point elevation constant for H2O is 0.512 °C/m.
You are a hazmat responder and walk into what appears to be a meth lab. There are flasks of iodine, White Gas fuel, Sodium Hydroxide, Nitric Acid, and a box of ephidrine.
What advantages and disadvantages exist for both organic and inorganic solar cells? Describe the main barriers or technical difficulties associated with each.
What volume, in liters, of O2 at 35°C and 1.19 atm can be produced from the decomposition of 10.0 g KNO3? 2 KNO3(s) → 2 KNO2(s) + O2(g)
How long would you need to sample from a concentration of 1000 PPM using a flow rate of 50 ml/minute to collect 100 mg of material?
The complex ion [Co(CN)6]^-3 absorbs a photon of wavelength 2.90×10^2 nm. What is the splitting energy of this complex?
What volume of hydrogen is necessary to react with five liters of nitrogen to produce ammonia?
Determine what is Δ[Br- ]/Δt If Δ[BrO 3 - ]/Δt = 0.018 M/s express your answer in M/s?
What is the net ionic equation for this reaction occurring in water: Potassium sulfate and barium chloride are mixed to form potassium
For the unbalanced equation _Al+_O2=_Al2O3. How many moles are needed to form 2.3 moles of aluminum oxide.
The solubility of silver sulfate in water is 0.223% (w/v) at 35°C. Calculate the solubility product of this salt at this temperature
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