Chemistry Answers

What is the molarity of Na+(aq) in a solution containing 0.250 M Na2SO4 (aq)?

How many moles of NaCl are contained in 328.0 mL of 2.81 M NaCl (aq)?

Zinc oxide can be produced by the following reaction:

2 Zn (s) + O2 (g) → 2 ZnO (s)

There are many uses for ZnO, but one is a heat-reflective coating on windows (thus lowering cooling demands in hot climates). This coating requires a thin layer (approximately 40-50 µm thick) of zinc oxide. 

  Assume that this thin film uses 1.9x1020 Zn atoms per cm2 of surface. How many grams of ZnO are added to a window that has an area of 5500 cm2?

In older airbags, sodium azide, NaN3, was used as a source of nitrogen gas to rapidly inflate the airbag. This practice was mostly discontinued due to the high toxicity of sodium azide. The reaction of interest is 2 NaN3 (s) → 2 Na (s) + 3 N2 (g) 

How many grams of N2 are produced if a 35.0 g charge of NaN3 decomposes?

Considering the same prompt, suppose I wanted to inflate a 125 L airbag with N2 (g) to a density of 0.450 g N2 / L. This is more or less a typical value for the passenger airbag. To do so I would need Answer g of N2 (g).

Considering the reaction for the decomposition of sodium azide, this would require a Answer g of NaN3.

This same process would produce Answer g Na (s). Keep in mind that sodium metal is highly reactive, and that a dose of ~ 2 g of sodium azide can be lethal. Sodium azide is still used in some airbags, but it has largely been phased out due to the legitimate safety concerns. 

 In older airbags, sodium azide, NaN₃, was used as a source of nitrogen gas to rapidly inflate the airbag. This practice was mostly discontinued due to the high toxicity of sodium azide. The reaction of interest is 2 NaN_3 (s) → 2 Na _(s) + 3 N_2 (g) 

How many grams of N₂ are produced if a 35.0 g charge of NaN₃ decomposes?

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A 400 mL buffer solution was prepared by reacting sodium acetate, CH₃COONa, with 1.00 M acetic acid, CH₃COOH, with a pH of 4.56 Calculate the mass of CH₃COONa required to prepare the solution. Ka CH₃COOH= 1.75 x 10^-5  

what is the percent hydrogen in ammonium oxalate (NH4)2C2O4

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1)  Many chemical processes release waste products into the atmosphere. Scientists are developing new solid catalysts to convert more efficiently these emissions into useful products, such as fuels. One example is a catalyst to convert these emissions into methanol. The catalyst is thought to work by breaking a H–H bond.

          An equation for this formation of methanol is given below.

          CO2(g) + 3H2(g) CH3OH(g) + H2O(g) ∆H = −49 kJ mol−1

(a)        Use the enthalpy change for the reaction and data on bond entahlpies to    calculate a value for the C=O bond enthalpy.