For each of the following balanced chemical equations, calculate how many moles and how many grams of each product would be produced by the complete conversion of 0.50 mole of the reactant indicated in boldface. state clearly the mole ratio used for each conversion. a. nh3(g) 1 hcl(g) s nh4cl(s)

Answer : The number of moles of and mass of is 0.50 mole and 27 grams respectively.

Solution : Given,

We are assuming that the reactant indicated in boldface is . So,

Moles of = 0.50 mole

Molar mass of = 53.5 g/mole

First we have to calculate the moles of

The balanced chemical reaction is,

From the reaction, we conclude that

As, 1 mole of react to give 1 mole of

So, 0.50 moles of react to give 0.50 moles of

The number of moles of  is, 0.50 moles.

Now we have to calculate the mass of

The mass of  is, 27 grams.

8

explanation:

each principal energy level above the first contains one s orbital and three p orbitals. a set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

mark brainliest and have a great day!

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.