In the equilibrium system below, which of the following changes would cause the equilibrium position to shift to the right? co(g) + 3h2 (g) two arrows stacked on top of each other. the top arrow points to the right. the bottom arrow points to the left. ch4 (g) + h2o (g) delta h = -206 kj/mol (2 points) decreasing the concentration of carbon monoxide (co) increasing the volume of the reaction system decreasing the concentration of hydrogen gas (h2) lowering the temperature of the reaction

We are given with the equation that produces methane and water from the raection of hydrogen gas and carbon monoxide. This is expressed in the balanced equation: 3H2 + CO = CH4 + H2O. This is an exothermic process. THE CHANGE THAT IS OCCURING IS LOWERING THE TEMPERATURE OF THE MINIMAL REACTION

when 25.0 ml of 0.700 mol/l naoh was mixed in a calorimeter with 25.0 ml of 0.700 mol/l hcl, both initially at 20.0 °c, the temperature increased to 22.1 °c. the heat capacity of the calorimeter is 279 j/°c.

the equation for the reaction is:

naoh + hcl → nacl + h₂o

moles of hcl = 0.0250 l hcl ×

0.700

mol hcl

1 l hcl = 0.0175 mol hcl

volume of solution = (25.0 + 25.0) ml = 50.0 ml

mass of solution = 50.0 ml soln ×

1.00

ml soln

= 50.0 g soln

δt=t2-t1

= (22.1 – 20.0) °c = 2.1 °c

the heats involved are

heat from neutralization + heat to warm solution + heat to warm calorimeter = 0

q1+q2+q3=0

nδh+mcδt+cδt=0

0.0175 mol ×

δh

+ 50.0 g × 4.184 j·g⁻¹°c⁻¹ × 2.1 °c + 279 j°c⁻¹ × 2.1 °c = 0

0.0175 mol ×

δh

+ 439.32 j + 585.9 j = 0

0.0175 mol ×

δh

= -1025.22 j

δh=1025.22j0.0175 mol= -58 600 j/mol = -58.6 kj/mol

narendra modi is currently the pm of india

explanation: