5. HS-PS1-4 Butane, C, H,, is the fuel found in barbeque lighters. When butane reacts with oxygen gas the following is the balanced chemical equation:
2 C. H.0 (1) + 13 02 (9) — 8 CO2 (g) + 10 H,0 (9)
The reaction releases energy in the form of heat and light. Which of the following statements is
the correct explanation for this reaction?
A. The energy required to break the bonds in the reactants are much greater than
the energy released when bonds are formed in the products, therefore this is an
endothermic reaction.
B. An energy input is NOT required to break bonds in the reactants and this
activation energy is released as heat and light.
C. Energy is absorbed when new bonds are formed in the products and this causes
the environment to heat up.
D. The energy released when the bonds formed in the products is greater than the
energy required to break the bonds in the reactants, therefore this is an
exothermic reaction.
E. The nuclei of each atom swaps their protons and neutrons and in the process
energy is released and this reaction is exothermic.

Idon't really understand this can you me and show your work.☺☺[ chemistry b] subject [ electron transfer in lonic bonds]grade( 12)

How many molecules are found in 1.32 mol of nacl?

Since the gas in your graduated cylinder is a mixture of butane and water vapor, you must determine the partial pressure of the butane, pbutane, alone. to do this, consult a reference and record the partial pressure of the water vapor, pwater, at the temperature you recorded. use the following formula to compute the partial pressure of the butane. pbutane = atmosphere - pwater use the following combined gas law formula and compute the volume that the butane sample will occupy at stp. (hint: convert both temperatures to kelvin.) pbutane x voriginal = pstandard x vfinal troom tstandard use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. grams of butane you used “x” grams of butane ml of butane corrected to stp = 22,400 ml compute the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table. compare your experimental results from #3 to the theoretical value of #4, computing a percent error of your findings using this formula: % error = measured value - accepted value x 100 accepted value use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. need asap