If 5.0 liters H2 (g) at STP is heated to a temperature of 985, pressure remaining constant, the new volume of the gas will be?

General Formulas and Concepts:

Chemistry - Gas Laws

STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 KCharles' Law:

Explanation:

Step 1: Define

Initial Volume: 5.0 L H₂ gas

Initial Temp: 273 K

Final Temp: 985 K

Final Volume: ?

Step 2: Solve for new volume

Substitute:                    Cross-multiply:             Multiply:                        Isolate x:                       Rewrite:                        

Step 3: Check

We are given 2 sig figs as the smallest. Follow sig fig rules and round.

It’s c it stays the same. and the atomic number goes up by 1. a neutron has changed into a proton plus an electron. the electron is emitted as a beta particle.

This is what i found on google “when one phosphate group is removed by breaking a phosphoanhydride bond in a process called hydrolysis, energy is released, and atp is converted to adenosine diphosphate (adp). likewise, energy is also released when a phosphate is removed from adp to form adenosine monophosphate (amp).” i hope this you .