Why are the soft types of wood not suitable a fuel in the smoking process?

Softwoods contain higher levels of air and sap, as they are a pine cone-producing species. So not only does the wood burn extremely fast, which is opposite of the “low and slow” barbecue practice, the flavors can be quite unpleasant and even toxic.

Pa brainliest po

a.) The mass of O₂ that will be needed to burn 36.1 g B₂H₆ is 125.29 g.

b.) There will be 1.39 moles of water produced from 19.2 g of B₂H₆.

Explanation:

This problem is an application of stoichiometry. Stoichiometry is a topic of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data or value.

In our case, the quantitative date we want is the a.) mass of oxygen (O₂) and b.) moles of water (H₂O) both from the reaction of diborane (B₂H₆) and oxygen (O₂).

Stoichiometry problems always need a balanced chemical reaction. In the problem, the chemical reaction is not yet balanced, meaning, we still need to balance the chemical equation reaction.

Balancing the chemical reaction we have:

B₂H₆ + O₂ → HBO₂ + H₂O

B₂H₆ + 3 O₂ → 2 HBO₂ + 2 H₂O

From the balanced chemical equation there are 2 moles of water forming from 1 mole of diborane, and 3 moles of oxygen is needed to react with 1 mole of diborane. These facts are to be used in order to solve the problem.

a.) Solving for the mass of oxygen from 36.1 grams of B₂H₆, we have:

(36.1 g B₂H₆) = 125.29 grams O₂

b.) Solving for moles of water from 19.2 grams of diborane, we have:

(19.2 g B₂H₆) = 1.39 mol H₂O

Note: 27.66 g B₂H₆ is from the molar mass of diboran, and 32 g/mole is from the molar mass of oxygen; these are necessary to use in order to cancel the units.

Hence, a.) There are 125.29 grams of O₂ needed to burn 36.1 g of B₂H₆, and b.) there will be 1.39 moles of water produced from 19.2 grams of B₂H₆.

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Good Day

Problem:

Ethane gas(C2H4) reacts with molecular oxygen gas to form carbon dioxide gas and liquid water, write the full balanced equation for this reaction with all states of matter labeled for each species.

Given:

                       C2H4    +    O2    →    CO2  +    H2O

Solution:

Balanced chemical equation:

         C2H4 (g)   +   3 O2 (g)    →    2 CO2 (g)  +   2 H2O (g)

                      C = 2                       C = 2

                      H = 4                        H = 4

                      O = 3 x 2 = 6            O = 4 + 2 = 6  

Hope it helps...=)